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Electrode Potentials

A-Level AQA Chemistry

This pack of flashcards encompasses principles of electrochemical cells, redox equilibria, standard electrode potentials, and calculation methods for electromotive force (EMF). It covers the roles and reactions of components in various types of cells, including hydrogen, nickel-cadmium, and lithium-ion, as well as the implications of changing conditions on cell potential.

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"Describe the effect of changing conditions on Ecell."	"Ecell is a measure of how far from equilibrium the cell reaction lies. The more positive the Ecell, the more likely the reaction is to occur."
"What is the effect of current flow on Ecell?"	"If current is allowed to flow, the cell reaction will occur and the Ecell will fall to zero as the reaction proceeds and the reactant concentrations drop."
"Define Le Chatelier's principle."	"Le Chatelier's principle states that if a system at equilibrium is subjected to a change in conditions, the system will adjust to minimize the effect of the change."
"How does increasing the concentration of reactants affect Ecell?"	"Increasing the concentration of reactants would increase Ecell."
"Describe the effect of temperature on Ecell."	"Most cells are exothermic in the spontaneous direction, so applying Le Chatelier's principle to a temperature rise would result in a decrease in Ecell."
"What are the different types of electrochemical cells?"	"Electrochemical cells can be non-rechargeable (irreversible), rechargeable, and fuel cells."
"What is the overall reaction for a dry cell?"	"Mn2O3 + 2NH3 + H2O + Zn2+ -> Ecell = +1.51V"
"Describe the purpose of secondary nickel-cadmium cells."	"Secondary nickel-cadmium cells are used to power electrical equipment such as drills and shavers."
"Explain why chlorine undergoes a redox reaction with water."	"Chlorine undergoes a redox reaction with water because it has a more positive electrode potential (E°) compared to the oxidation potential of water. This means that chlorine can oxidize water to produce oxygen gas."
"Describe the use of lithium ion cells."	"Lithium ion cells are used to power cameras and mobile phones."
"Explain the role of powdered graphite in lithium ion cells."	"Powdered graphite acts as a support medium in lithium ion cells, allowing the ions to react in the absence of a solvent like water."
"What is the purpose of fuel cells?"	"Fuel cells use the energy from the reaction of a fuel with oxygen to create a voltage."
"Describe the limitations of hydrogen fuel cells."	"Expensive, high production costs, limited lifetime, use of toxic chemicals in production."
"What are the advantages of fuel cells over conventional petrol or diesel-powered vehicles?"	"Less pollution, less CO2 emissions, greater efficiency."
"How can hydrogen be stored in fuel cells?"	"As a liquid under pressure, adsorbed on the surface of a solid material, absorbed within a solid material."
"Define electrolysis and its role in obtaining hydrogen."	"Electrolysis is the process of using electricity to split water into hydrogen and oxygen. It is used to obtain hydrogen for fuel cells."
"Describe the advantages of ethanol fuel cells compared to hydrogen fuel cells."	"Ethanol can be made from renewable sources, ethanol is less explosive and easier to store than hydrogen, no need for new petrol stations as ethanol is a liquid fuel."
"Define a secondary standard electrode."	"A secondary standard electrode is a standard electrode that has been calibrated against the primary standard (standard hydrogen electrode)."
"What is the purpose of a salt bridge in an electrochemical cell?"	"A salt bridge is used to connect the two half-cells in an electrochemical cell and allows for the flow of ions to maintain charge neutrality."
"Define electrode in the context of electrochemical cells."	"An electrode is a solid conductor (usually a metal) that facilitates the transfer of electrons between the electrolyte and the external circuit."
"How does a high resistance voltmeter prevent current flow in a circuit?"	"A high resistance voltmeter restricts the flow of current by offering a large resistance to the flow of electrons, preventing them from passing through the circuit."
"Describe what happens when current is allowed to flow in an electrochemical cell."	"When current flows in an electrochemical cell, the reactions occur separately at each electrode. The most positive electrode undergoes reduction, while the most negative electrode undergoes oxidation."
"What does the solid vertical line represent in a cell diagram?"	"The boundary between phases, such as solid (electrode) and solution (electrolyte)."
"Why is a platinum electrode used in systems that do not include metals?"	"A platinum electrode is used because it is unreactive and can conduct electricity."
"How is the more positive half cell represented in a cell diagram?"	"The more positive half cell is written on the right side of the cell diagram, if possible."
"Define electrode potential."	"Electrode potential is the potential difference between an electrode and a reference electrode, measured in volts."
"What is the purpose of a reference electrode in measuring electrode potential?"	"A reference electrode, such as the hydrogen electrode, is used to assign a relative potential of zero volts and compare it to other electrodes."
"Describe how the electrode potential of a half-cell is measured."	"The electrode potential of a half-cell is measured by connecting it to another half-cell of known potential and measuring the potential difference between the two half-cells."
"Describe the conditions required for the standard hydrogen electrode."	"The conditions required for the standard hydrogen electrode are hydrogen gas at a pressure of 100 kPa, a solution containing hydrogen ions at 1.0 mol dm-3, and a temperature of 298K."
"What are the common secondary standards used in place of the standard hydrogen electrode?"	"The common secondary standards used are silver/silver chloride electrode (E = +0.22 V) and calomel electrode (E = +0.27 V)."
"What is the purpose of a salt bridge in a cell with a standard hydrogen electrode?"	"The salt bridge is used to maintain electrical neutrality in the cell by allowing the flow of ions between the half-cells."
"Describe the equilibrium of the hydrogen electrode."	"The equilibrium of the hydrogen electrode is H2 (g) ⇌ 2H+ (aq) + 2e-. The hydrogen gas is oxidized to form hydrogen ions and electrons."
"Describe how to calculate the EMF of a cell."	"To calculate the EMF of a cell, use the equation Ecell = Erhs - Elhs, where Erhs is the electrode potential of the right-hand side half cell and Elhs is the electrode potential of the left-hand side half cell."
"What is the purpose of using electrode potentials in calculating the EMF of a cell?"	"The purpose of using electrode potentials is to determine the direction of spontaneous change for redox reactions."
"Define oxidation and reduction in terms of electrode potentials."	"Oxidation occurs at the more negative half cell, where electrons are given off (lost), while reduction occurs at the more positive half cell, where electrons are absorbed (gained)."
"Describe the relationship between electrode potentials and the direction of spontaneous change in a redox reaction."	"The more negative half cell will always oxidize (go backwards), while the more positive half cell will always reduce (go forwards). A spontaneous change will always have a positive Ecell."
"What is the significance of the series of standard electrode potentials?"	"The series of standard electrode potentials helps determine the strength of reducing and oxidizing agents. The most powerful reducing agents are found at the most negative end of the series, while the most powerful oxidizing agents are found at the most positive end."
"Describe why fluorine reacts with water."	"Fluorine reacts with because it has a more positive electrode potential (E°) compared to the oxidation potential of water. This means that fluorine can oxidize water to produce oxygen gas."

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Front

Describe the effect of changing conditions on Ecell.

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Ecell is a measure of how far from equilibrium the cell reaction lies. The more positive the Ecell, the more likely the reaction is to occur.

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[{"id":976526,"front":"Describe the effect of changing conditions on Ecell.","back":"Ecell is a measure of how far from equilibrium the cell reaction lies. The more positive the Ecell, the more likely the reaction is to occur.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Changing conditions can affect Ecell by altering the concentrations of reactants and products, temperature, and pressure. These changes can shift the equilibrium position of the cell reaction, resulting in a change in Ecell. Higher concentrations of reactants or lower concentrations of products can increase Ecell, making the reaction more likely to occur. Similarly, increasing temperature can increase Ecell, as higher temperatures generally favor reactions with positive ΔH values. Pressure changes may also impact Ecell, particularly in reactions involving gases.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976533,"front":"What is the effect of current flow on Ecell?","back":"If current is allowed to flow, the cell reaction will occur and the Ecell will fall to zero as the reaction proceeds and the reactant concentrations drop.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":1,"explanation":"When current flows in a cell, it indicates that the cell reaction is occurring. As the reaction proceeds, the concentrations of reactants decrease, causing the Ecell to decrease. This is because the driving force for the reaction decreases as reactants are consumed. Eventually, when the reactant concentrations drop to zero, the Ecell will reach zero as well.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976543,"front":"Define Le Chatelier's principle.","back":"Le Chatelier's principle states that if a system at equilibrium is subjected to a change in conditions, the system will adjust to minimize the effect of the change.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":2,"explanation":"Le Chatelier's principle is a fundamental concept in chemistry that explains how a system at equilibrium responds to changes in conditions. It states that when a change is applied to a system at equilibrium, the system will shift in a way that counteracts the change and restores equilibrium. This principle helps predict the direction in which a reaction will proceed when conditions are altered, such as changes in temperature, pressure, or concentration. By understanding Le Chatelier's principle, chemists can manipulate reaction conditions to optimize desired outcomes.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976549,"front":"How does increasing the concentration of reactants affect Ecell?","back":"Increasing the concentration of reactants would increase Ecell.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":3,"explanation":"Increasing the concentration of reactants affects Ecell because it changes the reaction quotient, Q. When reactant concentrations increase, Q becomes smaller, causing the cell potential to increase. This is due to the Nernst equation, which relates the cell potential to the concentrations of reactants and products.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976555,"front":"Describe the effect of temperature on Ecell.","back":"Most cells are exothermic in the spontaneous direction, so applying Le Chatelier's principle to a temperature rise would result in a decrease in Ecell.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":4,"explanation":"When temperature increases, the reaction rate typically increases due to increased kinetic energy of the reactant molecules. In an exothermic reaction, an increase in temperature would shift the equilibrium towards the reactants, resulting in a decrease in Ecell. This is because the reaction is releasing heat, and increasing the temperature would counteract this heat release by favoring the reactants.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976561,"front":"What are the different types of electrochemical cells?","back":"Electrochemical cells can be non-rechargeable (irreversible), rechargeable, and fuel cells.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":5,"explanation":"Electrochemical cells are devices that convert chemical energy into electrical energy. Non-rechargeable cells, also known as irreversible cells, are designed for one-time use. Rechargeable cells, on the other hand, can be recharged and reused multiple times. Fuel cells are a type of electrochemical cell that generate electricity through the continuous supply of fuel and an oxidant. These different types of cells offer various advantages and applications depending on their design and chemistry.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976567,"front":"What is the overall reaction for a dry cell?","back":"Mn2O3 + 2NH3 + H2O + Zn2+ -> Ecell = +1.51V","front_language":"English","back_language":"English","front_image":"","back_image":"","order":6,"explanation":"The overall reaction for a dry cell involves the reaction between manganese(III) oxide (Mn2O3), ammonia (NH3), water (H2O), and zinc ions (Zn2+). The cell potential (Ecell) for this reaction is +1.51V. This indicates that the reaction is spontaneous and can generate electrical energy. The specific details of the reaction mechanism and the role of each component are not provided in the answer.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976573,"front":"Describe the purpose of secondary nickel-cadmium cells.","back":"Secondary nickel-cadmium cells are used to power electrical equipment such as drills and shavers.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":7,"explanation":"Secondary nickel-cadmium cells are rechargeable batteries that are commonly used in various electrical equipment. They provide a reliable and long-lasting power source for devices such as drills and shavers. These cells can be recharged multiple times, making them cost-effective and environmentally friendly compared to disposable batteries. Additionally, nickel-cadmium cells have a high energy density, allowing them to store a significant amount of energy in a compact size. This makes them ideal for portable devices that require a reliable power source.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976506,"front":"Explain why chlorine undergoes a redox reaction with water.","back":"Chlorine undergoes a redox reaction with water because it has a more positive electrode potential (E°) compared to the oxidation potential of water. This means that chlorine can oxidize water to produce oxygen gas.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":8,"explanation":"Chlorine undergoes a redox reaction with water due to its higher electrode potential (E°) compared to water's oxidation potential. This indicates that chlorine can oxidize water, resulting in the production of oxygen gas. The redox reaction occurs as chlorine gains electrons from water, causing water to be oxidized while chlorine is reduced. This reaction is driven by the difference in electrode potentials between chlorine and water.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976592,"front":"Describe the use of lithium ion cells.","back":"Lithium ion cells are used to power cameras and mobile phones.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":9,"explanation":"Lithium ion cells are widely used in various electronic devices due to their high energy density, lightweight design, and long cycle life. They are commonly used to power portable devices such as cameras and mobile phones because they can provide a reliable and long-lasting source of energy. Additionally, lithium ion cells have a low self-discharge rate, allowing them to hold their charge for extended periods of time. This makes them ideal for applications where a rechargeable and compact power source is needed.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976599,"front":"Explain the role of powdered graphite in lithium ion cells.","back":"Powdered graphite acts as a support medium in lithium ion cells, allowing the ions to react in the absence of a solvent like water.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":10,"explanation":"Powdered graphite plays a crucial role in lithium ion cells by providing a medium for the ions to react. It acts as a support material, enabling the ions to undergo chemical reactions without the need for a solvent like water. This allows for efficient and safe operation of the lithium ion cells.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976603,"front":"What is the purpose of fuel cells?","back":"Fuel cells use the energy from the reaction of a fuel with oxygen to create a voltage.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":11,"explanation":"Fuel cells are devices that generate electricity through a chemical reaction between a fuel and oxygen. They are designed to convert chemical energy directly into electrical energy, without the need for combustion. This makes them more efficient and environmentally friendly compared to traditional combustion engines. Fuel cells have various applications, including powering vehicles, providing backup power, and generating electricity in remote areas. They offer a clean and sustainable alternative to fossil fuel-based power generation.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976608,"front":"Describe the limitations of hydrogen fuel cells.","back":"Expensive, high production costs, limited lifetime, use of toxic chemicals in production.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":12,"explanation":"Hydrogen fuel cells have limitations due to their expensive production costs, limited lifetime, and use of toxic chemicals. The high costs are mainly attributed to the materials used, such as platinum, which is needed as a catalyst. Additionally, the limited lifetime of fuel cells is due to the degradation of the catalyst over time. The production process also involves the use of toxic chemicals, which can have environmental and health implications. These limitations need to be addressed for wider adoption of hydrogen fuel cells.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976613,"front":"What are the advantages of fuel cells over conventional petrol or diesel-powered vehicles?","back":"Less pollution, less CO2 emissions, greater efficiency.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":13,"explanation":"Fuel cells have several advantages over conventional petrol or diesel-powered vehicles. Firstly, they produce less pollution, as they do not emit harmful pollutants such as nitrogen oxides or particulate matter. Secondly, fuel cells have lower CO2 emissions, as they use hydrogen or other clean fuels. Lastly, fuel cells are more efficient, as they convert fuel directly into electricity without the need for combustion, resulting in less energy waste.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976616,"front":"How can hydrogen be stored in fuel cells?","back":"As a liquid under pressure, adsorbed on the surface of a solid material, absorbed within a solid material.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":14,"explanation":"Hydrogen can be stored in fuel cells in different ways. One method is by compressing it into a liquid state under high pressure. Another way is by adsorbing it onto the surface of a solid material, which increases its storage capacity. Additionally, hydrogen can be absorbed within a solid material, allowing for safe and efficient storage. These storage methods ensure a reliable and convenient supply of hydrogen for fuel cells.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976619,"front":"Define electrolysis and its role in obtaining hydrogen.","back":"Electrolysis is the process of using electricity to split water into hydrogen and oxygen. It is used to obtain hydrogen for fuel cells.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":15,"explanation":"Electrolysis is a chemical process that uses an electric current to break down a compound, in this case water, into its constituent elements, hydrogen and oxygen. By passing an electric current through water, the water molecules are dissociated, resulting in the release of hydrogen gas at the cathode and oxygen gas at the anode. This method is commonly used to obtain hydrogen for various applications, including fuel cells, where hydrogen is used as a clean and efficient source of energy.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976622,"front":"Describe the advantages of ethanol fuel cells compared to hydrogen fuel cells.","back":"Ethanol can be made from renewable sources, ethanol is less explosive and easier to store than hydrogen, no need for new petrol stations as ethanol is a liquid fuel.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":16,"explanation":"Ethanol fuel cells have several advantages over hydrogen fuel cells. Firstly, ethanol can be produced from renewable sources, making it a more sustainable option. Additionally, ethanol is less explosive and easier to store than hydrogen, reducing safety concerns. Furthermore, the existing infrastructure for liquid fuel can be utilized for ethanol, eliminating the need for new petrol stations. These advantages make ethanol fuel cells a promising alternative to hydrogen fuel cells.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976466,"front":"Define a secondary standard electrode.","back":"A secondary standard electrode is a standard electrode that has been calibrated against the primary standard (standard hydrogen electrode).","front_language":"English","back_language":"English","front_image":"","back_image":"","order":17,"explanation":"A secondary standard electrode is a calibrated electrode that is used as a reference in electrochemical measurements. It is calibrated against the primary standard electrode, which is the standard hydrogen electrode. The secondary standard electrode allows for accurate and reliable measurements by providing a known reference potential.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976435,"front":"What is the purpose of a salt bridge in an electrochemical cell?","back":"A salt bridge is used to connect the two half-cells in an electrochemical cell and allows for the flow of ions to maintain charge neutrality.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":18,"explanation":"The purpose of a salt bridge in an electrochemical cell is to maintain charge neutrality. It achieves this by allowing the flow of ions between the two half-cells. Without a salt bridge, the buildup of charge in one half-cell would prevent the flow of electrons and halt the cell's operation. The salt bridge ensures a continuous flow of ions, enabling the cell to function properly.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976437,"front":"Define electrode in the context of electrochemical cells.","back":"An electrode is a solid conductor (usually a metal) that facilitates the transfer of electrons between the electrolyte and the external circuit.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":19,"explanation":"In electrochemical cells, electrodes play a crucial role in facilitating electron transfer between the electrolyte and the external circuit. They are typically made of solid conductors, often metals. By providing a surface for electron exchange, electrodes enable the flow of current in the cell. This transfer of electrons is essential for the chemical reactions that occur within the cell, allowing for the conversion of chemical energy into electrical energy or vice versa.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976439,"front":"How does a high resistance voltmeter prevent current flow in a circuit?","back":"A high resistance voltmeter restricts the flow of current by offering a large resistance to the flow of electrons, preventing them from passing through the circuit.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":20,"explanation":"A high resistance voltmeter prevents current flow in a circuit because it acts as a barrier to the flow of electrons. By offering a large resistance, it limits the amount of current that can pass through it. This restriction ensures that the majority of the current flows through the circuit being measured, allowing the voltmeter to accurately measure the voltage without interfering with the circuit's operation.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976441,"front":"Describe what happens when current is allowed to flow in an electrochemical cell.","back":"When current flows in an electrochemical cell, the reactions occur separately at each electrode. The most positive electrode undergoes reduction, while the most negative electrode undergoes oxidation.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":21,"explanation":"When current flows in an electrochemical cell, it causes separate reactions to occur at each electrode. The electrode with the highest potential undergoes reduction, which involves the gain of electrons. Conversely, the electrode with the lowest potential undergoes oxidation, which involves the loss of electrons. This flow of electrons allows for the transfer of charge and the generation of electrical energy in the cell.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976443,"front":"What does the solid vertical line represent in a cell diagram?","back":"The boundary between phases, such as solid (electrode) and solution (electrolyte).","front_language":"English","back_language":"English","front_image":"","back_image":"","order":22,"explanation":"The solid vertical line in a cell diagram represents the boundary between different phases within the cell. It specifically indicates the separation between the solid electrode and the solution electrolyte. This line is crucial in understanding the different components and their interactions within the cell.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976446,"front":"Why is a platinum electrode used in systems that do not include metals?","back":"A platinum electrode is used because it is unreactive and can conduct electricity.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":23,"explanation":"Platinum is chosen as an electrode in non-metal systems due to its unreactive nature and excellent electrical conductivity. Its unreactivity ensures that it does not interfere with the chemical reactions occurring in the system. Additionally, platinum's high electrical conductivity allows for efficient transfer of electrons, enabling accurate measurements and efficient functioning of the system.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976452,"front":"How is the more positive half cell represented in a cell diagram?","back":"The more positive half cell is written on the right side of the cell diagram, if possible.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":24,"explanation":"In a cell diagram, the more positive half cell is typically represented on the right side. This is because the direction of electron flow is from the more negative to the more positive electrode. By placing the more positive half cell on the right, it indicates the direction of electron flow in the diagram.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976453,"front":"Define electrode potential.","back":"Electrode potential is the potential difference between an electrode and a reference electrode, measured in volts.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":25,"explanation":"Electrode potential is a measure of the tendency of an electrode to gain or lose electrons during a redox reaction. It is influenced by factors such as the nature of the electrode material, the concentration of ions in the solution, and temperature. The reference electrode is used as a standard to measure the potential difference. The unit of measurement for electrode potential is volts, which represents the energy per unit charge.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976456,"front":"What is the purpose of a reference electrode in measuring electrode potential?","back":"A reference electrode, such as the hydrogen electrode, is used to assign a relative potential of zero volts and compare it to other electrodes.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":26,"explanation":"The purpose of a reference electrode in measuring electrode potential is to establish a baseline or reference point for comparison. By using a reference electrode, such as the hydrogen electrode, which has a known and stable potential of zero volts, the potential of other electrodes can be measured relative to this reference. This allows for accurate and standardized comparisons between different electrodes and their potentials.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976458,"front":"Describe how the electrode potential of a half-cell is measured.","back":"The electrode potential of a half-cell is measured by connecting it to another half-cell of known potential and measuring the potential difference between the two half-cells.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":27,"explanation":"The electrode potential of a half-cell is measured by comparing it to another half-cell of known potential. This is done by connecting the two half-cells and measuring the potential difference between them. By comparing the potentials, the electrode potential of the unknown half-cell can be determined. This method allows for the quantification of the relative tendency of a half-cell to gain or lose electrons.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976471,"front":"Describe the conditions required for the standard hydrogen electrode.","back":"The conditions required for the standard hydrogen electrode are hydrogen gas at a pressure of 100 kPa, a solution containing hydrogen ions at 1.0 mol dm-3, and a temperature of 298K.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":28,"explanation":"The standard hydrogen electrode requires specific conditions to function properly. These include a specific pressure of hydrogen gas, a solution with a specific concentration of hydrogen ions, and a specific temperature. These conditions are necessary to ensure accurate and consistent measurements when using the standard hydrogen electrode in electrochemical experiments.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976474,"front":"What are the common secondary standards used in place of the standard hydrogen electrode?","back":"The common secondary standards used are silver/silver chloride electrode (E = +0.22 V) and calomel electrode (E = +0.27 V).","front_language":"English","back_language":"English","front_image":"","back_image":"","order":29,"explanation":"The silver/silver chloride electrode and calomel electrode are commonly used as secondary standards instead of the standard hydrogen electrode. These electrodes have known and stable potentials, with the silver/silver chloride electrode having a potential of +0.22 V and the calomel electrode having a potential of +0.27 V. They are used as reference electrodes in various electrochemical measurements and experiments.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976477,"front":"What is the purpose of a salt bridge in a cell with a standard hydrogen electrode?","back":"The salt bridge is used to maintain electrical neutrality in the cell by allowing the flow of ions between the half-cells.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":30,"explanation":"The purpose of a salt bridge in a cell with a standard hydrogen electrode is to maintain electrical neutrality. It achieves this by allowing the flow of ions between the half-cells. This is important because in a redox reaction, electrons are transferred from one half-cell to another, and without a salt bridge, the buildup of charge would prevent further electron transfer. The salt bridge ensures a continuous flow of ions, allowing the reaction to proceed smoothly.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976479,"front":"Describe the equilibrium of the hydrogen electrode.","back":"The equilibrium of the hydrogen electrode is H2 (g) ⇌ 2H+ (aq) + 2e-. The hydrogen gas is oxidized to form hydrogen ions and electrons.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":31,"explanation":"The equilibrium of the hydrogen electrode involves the oxidation of hydrogen gas to form hydrogen ions and electrons. This process occurs at the interface between the gas phase (H2) and the aqueous phase (H+). The electrode potential of the hydrogen electrode is used as a reference in many electrochemical measurements.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976483,"front":"Describe how to calculate the EMF of a cell.","back":"To calculate the EMF of a cell, use the equation Ecell = Erhs - Elhs, where Erhs is the electrode potential of the right-hand side half cell and Elhs is the electrode potential of the left-hand side half cell.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":32,"explanation":"The EMF of a cell can be calculated by subtracting the electrode potential of the left-hand side half cell from the electrode potential of the right-hand side half cell. This equation, Ecell = Erhs - Elhs, allows us to determine the overall potential difference generated by the cell. The electrode potential is a measure of the tendency of an electrode to gain or lose electrons, and it is influenced by factors such as the nature of the electrode material and the concentration of species involved in the redox reaction. By subtracting the potential of the left-hand side from the right-hand side, we can determine the net potential difference across the cell.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976485,"front":"What is the purpose of using electrode potentials in calculating the EMF of a cell?","back":"The purpose of using electrode potentials is to determine the direction of spontaneous change for redox reactions.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":33,"explanation":"Electrode potentials are used to determine the direction of spontaneous change in redox reactions. This is because the potential difference between two electrodes in a cell indicates the tendency for electrons to flow from one electrode to another. By comparing the electrode potentials, we can determine which electrode will undergo oxidation and which will undergo reduction, and therefore predict the direction of the overall reaction.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976488,"front":"Define oxidation and reduction in terms of electrode potentials.","back":"Oxidation occurs at the more negative half cell, where electrons are given off (lost), while reduction occurs at the more positive half cell, where electrons are absorbed (gained).","front_language":"English","back_language":"English","front_image":"","back_image":"","order":34,"explanation":"Oxidation and reduction are fundamental processes in electrochemistry. Oxidation involves the loss of electrons, which occurs at the more negative half cell. Reduction, on the other hand, involves the gain of electrons and takes place at the more positive half cell. These processes are driven by the difference in electrode potentials between the two half cells. The more negative the potential, the greater the tendency for oxidation to occur, while the more positive the potential, the greater the tendency for reduction to occur.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976492,"front":"Describe the relationship between electrode potentials and the direction of spontaneous change in a redox reaction.","back":"The more negative half cell will always oxidize (go backwards), while the more positive half cell will always reduce (go forwards). A spontaneous change will always have a positive Ecell.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":35,"explanation":"The relationship between electrode potentials and the direction of spontaneous change in a redox reaction is determined by the difference in potential between the two half-cells. The half-cell with a more negative potential will undergo oxidation, while the half-cell with a more positive potential will undergo reduction. This directionality ensures that the reaction proceeds spontaneously. The overall cell potential, known as Ecell, will be positive for a spontaneous change.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976495,"front":"What is the significance of the series of standard electrode potentials?","back":"The series of standard electrode potentials helps determine the strength of reducing and oxidizing agents. The most powerful reducing agents are found at the most negative end of the series, while the most powerful oxidizing agents are found at the most positive end.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":36,"explanation":"The series of standard electrode potentials is significant because it allows us to rank the strength of reducing and oxidizing agents. It provides a quantitative measure of the tendency of a species to gain or lose electrons. The more negative the standard electrode potential, the stronger the reducing agent, while the more positive the potential, the stronger the oxidizing agent. This information is crucial in understanding and predicting redox reactions and their feasibility.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":976499,"front":"Describe why fluorine reacts with water.","back":"Fluorine reacts with because it has a more positive electrode potential (E°) compared to the oxidation potential of water. This means that fluorine can oxidize water to produce oxygen gas.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":37,"explanation":"Fluorine reacts with water due to its high electrode potential (E°) compared to the oxidation potential of water. This means that fluorine can easily oxidize water molecules, leading to the production of oxygen gas. The high reactivity of fluorine is attributed to its strong electronegativity, which allows it to attract electrons from water molecules and form stable compounds. This reaction is highly exothermic and can be explosive in nature.","deleted_at":null,"flashcard_deck_id":"hKnDg","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}}]

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