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Rate Equations

A-Level AQA Chemistry

This pack of flashcards covers the principles of chemical kinetics, focusing on the rate equation, reaction orders, and experimental determination of reaction rates. It includes the significance of reactant concentration, initial rate method, clock reactions, and temperature's effect on rate constants, as well as the Arrhenius equation and reaction mechanisms.

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"Describe the unit of the Arrhenius constant A."	"The unit of the Arrhenius constant A will be the same as the unit of the rate constant k."
"How does the rate change when the concentration of reactant X doubles?"	"When the concentration of reactant X doubles, the rate also doubles."
"What is the overall order of the reaction?"	"The overall order of the reaction is third order."
"How does increasing the temperature affect the value of the rate constant?"	"Increasing the temperature increases the value of the rate constant."
"Define zero order reaction."	"A zero order reaction is a reaction in which the rate stays constant as the reactant is used up."
"What is the value of the rate constant for a zero order reaction?"	"The value of the rate constant for a zero order reaction is equal to the gradient of the concentration-time graph."
"Describe the relationship between the concentration of a reactant and the rate in a zero order reaction."	"In a zero order reaction, the concentration of a reactant has no effect on the rate."
"Describe the effect of temperature on the rate constant."	"Increasing the temperature increases the value of the rate constant k."
"Define the Arrhenius equation."	"The Arrhenius equation is given by k = Ae-EA/RT, where A is the Arrhenius constant, R is the gas constant, and EA is activation energy."
"What is the unit of temperature in the Arrhenius equation?"	"The unit of temperature in the Arrhenius equation is Kelvin (K)."
"How is the Arrhenius equation usually rearranged?"	"The Arrhenius equation is usually rearranged to Ink=InA-EA/RT."
"Describe the units of activation energy."	"Activation energy should be in J mol-¹ to match the units of R."
"Do you need to know how to rearrange the Arrhenius equation?"	"Yes, you should be able to do rearrangements and substitute values into both the original and rearranged equations."
"What is the rate equation for the reaction between X and Y?"	"The rate equation for the reaction between X and Y is r = k [X][Y]^2."
"Describe how to calculate the activation energy graphically from experimental data."	"Plot a graph of ln(rate) or ln(k) against 1/T. Measure the gradient of the line and multiply it by the gas constant (R) to obtain the activation energy (EA)."
"What is the relationship between the rate constant (k) and the rate of reaction?"	"The rate constant (k) is proportional to the rate of reaction."
"Define activation energy (EA)."	"Activation energy (EA) is the minimum energy required for a chemical reaction to occur."
"How can the activation energy be calculated using the graph?"	"The activation energy can be calculated by measuring the gradient of the ln(rate) or ln(k) versus 1/T graph."
"Describe the unit of activation energy (EA) obtained using the given equation."	"The unit of activation energy (EA) obtained using the given equation is J mol-¹. It can be converted to kJ mol-1 by dividing by 1000."
"Describe a rate-determining step in a reaction mechanism."	"The rate-determining step is the slowest step in a reaction mechanism and controls the overall rate of the reaction."
"Define molecularity in the context of a reaction mechanism."	"Molecularity refers to the number of moles of each substance involved in the slowest step of a reaction mechanism."
"What is the order of reaction for a substance if it appears as 0 moles in the slow step of a reaction mechanism?"	"If a substance appears as 0 moles in the slow step, it is considered to be zero order."
"How can the rate equation be modified when an intermediate compound is involved in a reaction mechanism?"	"The rate equation must be modified to include the substances that make up the intermediate compound in a previous step of the mechanism."
"Describe the Sn2 mechanism in nucleophilic substitution reactions."	"The Sn2 mechanism is a one-step mechanism where the nucleophile attacks the substrate at the same time as the leaving group departs."
"How can the change in volume of a gas be measured to determine the rate of reaction?"	"The change in volume of a gas can be measured using a gas syringe. This method is suitable for measuring continuous rate, but the gas syringe typically measures up to 100ml of gas."
"What does the symbol 'r' represent in the rate equation?"	"The symbol 'r' represents the rate of reaction."
"What do the square brackets '[A]' mean in the rate equation?"	"The square brackets '[A]' represent the concentration of reactant A."
"What is the unit of 'r' in the rate equation?"	"The unit of 'r' is usually mol dm-3 s-1."
"What is the rate constant 'k' in the rate equation?"	"The rate constant 'k' is a proportionality constant that relates the rate of reaction to the concentration of reactants."
"What is the total order for a reaction?"	"The total order for a reaction is determined by adding all the individual reaction orders together."
"How are the reaction orders determined?"	"The reaction orders are determined experimentally and are not the same as the stoichiometric coefficients in the balanced equation."
"How can the unit of k be calculated?"	"The unit of k can be calculated by rearranging the rate equation, inserting the units, and simplifying the fraction."
"Describe the concept of continuous monitoring in relation to rate of reaction."	"Continuous monitoring refers to following one experiment over time and recording the change in concentration. The gradient of the concentration-time graph represents the rate of reaction."
"What is the significance of having a large excess of reactants in a reaction?"	"In reactions with several reactants, if one reactant is kept in a large excess, it will appear to have no effect on the rate and will be pseudo-zero order. This is because its concentration stays virtually constant and does not affect the rate."
"What is a common clock reaction?"	"A common clock reaction involves two successive reactions, where the end point is achieved when one limited reactant runs out, resulting in a sudden color change."
"How can the order of reaction be determined in a clock reaction?"	"By repeating the experiment several times and varying the concentration of a reactant while keeping the other reactants at constant concentration, the order of reaction with respect to that reactant can be determined."
"How can the of a reaction be calculated graphically?"	"By plotting a graph of log rate vs log [Y], where Y is the concentration of one of the reactants that is changed, the gradient of the line obtained is equal to the order of the reaction."
"Define the term 'order' in the context of a rate equation."	"The order of a reactant in a rate equation represents the power to which its concentration is raised in the rate equation."
"What is the significance of high concentrations and quick times in experimental initial rate data?"	"High concentrations and quick times in experiments can lead to the biggest percentage errors in the initial rate data."
"Describe the effect of changing the concentration of both reactants simultaneously on the rate of a reaction."	"The effect of changing the concentration of both reactants simultaneously is that the individual changes in concentration are multiplied together to give an overall change in the rate of the reaction."

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Describe the unit of the Arrhenius constant A.

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The unit of the Arrhenius constant A will be the same as the unit of the rate constant k.

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[{"id":974961,"front":"Describe the unit of the Arrhenius constant A.","back":"The unit of the Arrhenius constant A will be the same as the unit of the rate constant k.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The Arrhenius constant A is a proportionality constant that relates the rate constant of a chemical reaction to the temperature. It represents the frequency of successful collisions between reactant molecules. The unit of A is determined by the unit of the rate constant k, which is dependent on the overall reaction order. Therefore, the unit of A will vary depending on the specific reaction being studied.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974949,"front":"How does the rate change when the concentration of reactant X doubles?","back":"When the concentration of reactant X doubles, the rate also doubles.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":1,"explanation":"When the concentration of a reactant doubles, it means that there are now twice as many molecules of that reactant available for the reaction. This leads to an increase in the frequency of collisions between reactant molecules, resulting in a higher rate of reaction. 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This information helps to understand how changes in reactant concentrations will affect the rate of the reaction.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974951,"front":"How does increasing the temperature affect the value of the rate constant?","back":"Increasing the temperature increases the value of the rate constant.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":3,"explanation":"Increasing the temperature affects the value of the rate constant because it speeds up the rate of reaction. This is due to the fact that higher temperatures provide more energy to the reactant molecules, allowing them to overcome the activation energy barrier more easily. As a result, the rate constant increases, indicating a faster reaction rate.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974952,"front":"Define zero order reaction.","back":"A zero order reaction is a reaction in which the rate stays constant as the reactant is used up.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":4,"explanation":"A zero order reaction is characterized by a constant rate of reaction, regardless of the concentration of the reactant. This is because the rate-determining step is independent of the reactant concentration. In other words, the reaction proceeds at a fixed rate, unaffected by changes in reactant concentration. This behavior is often observed when the reaction is catalyzed by a catalyst or when the reaction is limited by a surface area or enzyme activity.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974953,"front":"What is the value of the rate constant for a zero order reaction?","back":"The value of the rate constant for a zero order reaction is equal to the gradient of the concentration-time graph.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":5,"explanation":"In a zero order reaction, the rate of the reaction is independent of the concentration of the reactant. This means that the rate constant, which represents the speed of the reaction, remains constant throughout the reaction. The gradient of the concentration-time graph represents the rate of change of concentration over time, and in a zero order reaction, this gradient is equal to the rate constant.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974954,"front":"Describe the relationship between the concentration of a reactant and the rate in a zero order reaction.","back":"In a zero order reaction, the concentration of a reactant has no effect on the rate.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":6,"explanation":"In a zero order reaction, the rate of the reaction is independent of the concentration of the reactant. This means that even if the concentration of the reactant increases or decreases, the rate of the reaction remains constant. The rate is determined solely by other factors such as temperature, catalysts, or the presence of other reactants. This is in contrast to other reaction orders where the rate is directly proportional to the concentration of the reactant.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974955,"front":"Describe the effect of temperature on the rate constant.","back":"Increasing the temperature increases the value of the rate constant k.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":7,"explanation":"Increasing the temperature has a direct effect on the rate constant. This is because temperature affects the kinetic energy of molecules, leading to more frequent and energetic collisions. As a result, the reaction rate increases, causing the rate constant to increase as well. This relationship is described by the Arrhenius equation, which shows that the rate constant is exponentially dependent on temperature.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974956,"front":"Define the Arrhenius equation.","back":"The Arrhenius equation is given by k = Ae-EA/RT, where A is the Arrhenius constant, R is the gas constant, and EA is activation energy.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":8,"explanation":"The Arrhenius equation is a mathematical expression that relates the rate constant (k) of a chemical reaction to the temperature (T) and activation energy (EA). It shows that as temperature increases, the rate of reaction also increases. The equation includes the Arrhenius constant (A), which represents the frequency of collisions between reactant molecules. The exponential term, e^(-EA/RT), accounts for the fraction of molecules with sufficient energy to overcome the activation energy barrier. Overall, the Arrhenius equation provides a quantitative understanding of how temperature affects reaction rates.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974957,"front":"What is the unit of temperature in the Arrhenius equation?","back":"The unit of temperature in the Arrhenius equation is Kelvin (K).","front_language":"English","back_language":"English","front_image":"","back_image":"","order":9,"explanation":"The unit of temperature in the Arrhenius equation is Kelvin (K) because it is an absolute temperature scale commonly used in scientific calculations. The Arrhenius equation describes the temperature dependence of reaction rates, and using Kelvin ensures consistency with thermodynamic principles.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974958,"front":"How is the Arrhenius equation usually rearranged?","back":"The Arrhenius equation is usually rearranged to Ink=InA-EA/RT.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":10,"explanation":"The Arrhenius equation is typically rearranged to solve for the natural logarithm of the rate constant (ln k). This rearrangement allows for the determination of the activation energy (Ea) and the pre-exponential factor (A) from experimental data. It simplifies the relationship between reaction rate and temperature.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974959,"front":"Describe the units of activation energy.","back":"Activation energy should be in J mol-¹ to match the units of R.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":11,"explanation":"Activation energy is a crucial concept in chemistry, representing the minimum energy required for a reaction to occur. The use of J mol⁻¹ aligns with the universal gas constant (R), which is often expressed in these units. This consistency is essential for accurate calculations in thermodynamics and kinetics.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974960,"front":"Do you need to know how to rearrange the Arrhenius equation?","back":"Yes, you should be able to do rearrangements and substitute values into both the original and rearranged equations.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":12,"explanation":"Understanding how to rearrange the Arrhenius equation is crucial in various scientific fields like chemistry and physics. It allows for manipulating the equation to solve for different variables, aiding in calculations and analysis. Being proficient in rearranging equations enhances problem-solving skills and comprehension of underlying principles.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974948,"front":"What is the rate equation for the reaction between X and Y?","back":"The rate equation for the reaction between X and Y is r = k [X][Y]^2.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":13,"explanation":"The rate equation for a chemical reaction describes the relationship between the rate of the reaction and the concentrations of the reactants. In this case, the rate equation indicates that the rate of the reaction is directly proportional to the concentration of X and to the square of the concentration of Y, with the proportionality constant k representing the rate constant. This means that as the concentrations of X and Y increase, the rate of the reaction will also increase.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974964,"front":"Describe how to calculate the activation energy graphically from experimental data.","back":"Plot a graph of ln(rate) or ln(k) against 1/T. Measure the gradient of the line and multiply it by the gas constant (R) to obtain the activation energy (EA).","front_language":"English","back_language":"English","front_image":"","back_image":"","order":14,"explanation":"The method described involves using the Arrhenius equation to plot a graph of ln(rate) or ln(k) against 1/T. The gradient of the resulting line represents -Ea/R, allowing the activation energy (Ea) to be calculated by multiplying the gradient by the gas constant (R). This graphical approach provides a straightforward means of determining activation energy from experimental data.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974965,"front":"What is the relationship between the rate constant (k) and the rate of reaction?","back":"The rate constant (k) is proportional to the rate of reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":15,"explanation":"The rate constant (k) reflects how quickly a reaction occurs at a given temperature and concentration. A higher k indicates a faster reaction, while a lower k suggests a slower one. This relationship is crucial for understanding reaction dynamics and predicting how changes in conditions affect reaction speed.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974966,"front":"Define activation energy (EA).","back":"Activation energy (EA) is the minimum energy required for a chemical reaction to occur.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":16,"explanation":"Activation energy (EA) is crucial in determining the rate of a chemical reaction. It represents the energy barrier that reactant molecules must overcome for the reaction to proceed. Higher EA values indicate slower reactions, while lower EA values indicate faster reactions.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974967,"front":"How can the activation energy be calculated using the graph?","back":"The activation energy can be calculated by measuring the gradient of the ln(rate) or ln(k) versus 1/T graph.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":17,"explanation":"The activation energy is determined by analyzing the slope of the natural logarithm of the reaction rate or rate constant plotted against the reciprocal of temperature. This relationship is based on the Arrhenius equation, which describes the temperature dependence of reaction rates.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974968,"front":"Describe the unit of activation energy (EA) obtained using the given equation.","back":"The unit of activation energy (EA) obtained using the given equation is J mol-¹. It can be converted to kJ mol-1 by dividing by 1000.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":18,"explanation":"Activation energy (EA) is a measure of the energy barrier that must be overcome for a chemical reaction to occur. It is typically expressed in joules per mole (J mol⁻¹) but can also be converted to kilojoules per mole (kJ mol⁻¹) by dividing by 1000. This unit helps quantify the energy required for a reaction to proceed.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974969,"front":"Describe a rate-determining step in a reaction mechanism.","back":"The rate-determining step is the slowest step in a reaction mechanism and controls the overall rate of the reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":19,"explanation":"In a reaction mechanism, the rate-determining step is crucial because it acts as a bottleneck, influencing how quickly the entire process can proceed. Understanding this step helps chemists optimize conditions and design catalysts, ultimately improving reaction efficiency and yield in various applications.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974970,"front":"Define molecularity in the context of a reaction mechanism.","back":"Molecularity refers to the number of moles of each substance involved in the slowest step of a reaction mechanism.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":20,"explanation":"Molecularity is a crucial concept in understanding reaction mechanisms as it directly relates to the number of molecules that participate in the rate-determining step. This parameter helps determine the overall reaction rate and sheds light on the complexity of the reaction pathway.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974971,"front":"What is the order of reaction for a substance if it appears as 0 moles in the slow step of a reaction mechanism?","back":"If a substance appears as 0 moles in the slow step, it is considered to be zero order.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":21,"explanation":"In a reaction mechanism, the slow step determines the overall rate. If a substance doesn't affect the rate because it doesn't appear in the slow step, it's considered to be zero order. This means its concentration doesn't impact the reaction rate, making it zero order.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974972,"front":"How can the rate equation be modified when an intermediate compound is involved in a reaction mechanism?","back":"The rate equation must be modified to include the substances that make up the intermediate compound in a previous step of the mechanism.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":22,"explanation":"In reactions involving intermediates, the rate law reflects the slowest step, often the rate-determining step. Since intermediates are not present in the overall reaction, their concentrations must be expressed in terms of reactants or products from earlier steps, ensuring the rate equation accurately represents the reaction dynamics.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974973,"front":"Describe the Sn2 mechanism in nucleophilic substitution reactions.","back":"The Sn2 mechanism is a one-step mechanism where the nucleophile attacks the substrate at the same time as the leaving group departs.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":23,"explanation":"The Sn2 mechanism involves a backside attack by the nucleophile on the electrophilic center, leading to inversion of stereochemistry. It is favored in primary substrates due to less steric hindrance. The leaving group departure and nucleophile attack occur simultaneously, resulting in a concerted reaction.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974934,"front":"How can the change in volume of a gas be measured to determine the rate of reaction?","back":"The change in volume of a gas can be measured using a gas syringe. This method is suitable for measuring continuous rate, but the gas syringe typically measures up to 100ml of gas.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":24,"explanation":"Using a gas syringe allows for precise measurement of gas volume changes during a reaction, providing real-time data on reaction rates. This method is particularly effective for reactions producing gases, as it directly correlates volume change with reaction progress, enhancing accuracy in kinetic studies.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974910,"front":"What does the symbol 'r' represent in the rate equation?","back":"The symbol 'r' represents the rate of reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":25,"explanation":"In chemical kinetics, the rate of reaction is crucial for understanding how quickly reactants convert to products. It can be influenced by factors such as concentration, temperature, and catalysts. The rate provides insight into the reaction mechanism and helps in optimizing conditions for desired outcomes.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974913,"front":"What do the square brackets '[A]' mean in the rate equation?","back":"The square brackets '[A]' represent the concentration of reactant A.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":26,"explanation":"Square brackets in a rate equation indicate the molarity of a substance, which is crucial for understanding reaction kinetics. Concentration directly influences reaction rates; higher concentrations typically lead to more frequent collisions between reactant molecules, thus accelerating the reaction.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974917,"front":"What is the unit of 'r' in the rate equation?","back":"The unit of 'r' is usually mol dm-3 s-1.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":27,"explanation":"In chemical kinetics, 'r' represents the rate of a reaction, indicating how quickly reactants are converted into products. The unit mol dm-3 s-1 reflects the change in concentration (moles per cubic decimeter) over time (seconds), providing a clear measure of reaction speed in a given volume.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974921,"front":"What is the rate constant 'k' in the rate equation?","back":"The rate constant 'k' is a proportionality constant that relates the rate of reaction to the concentration of reactants.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":28,"explanation":"The rate constant 'k' is crucial in chemical kinetics as it provides insight into the speed of a reaction under specific conditions. It varies with temperature and can indicate the reaction's mechanism. A higher 'k' suggests a faster reaction, while its units depend on the overall order of the reaction.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974923,"front":"What is the total order for a reaction?","back":"The total order for a reaction is determined by adding all the individual reaction orders together.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":29,"explanation":"Total order reflects the sum of the powers of the concentration terms in the rate law, indicating how the rate of reaction depends on the concentration of reactants. It provides insight into the reaction mechanism and can influence the design of experiments and industrial processes.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974924,"front":"How are the reaction orders determined?","back":"The reaction orders are determined experimentally and are not the same as the stoichiometric coefficients in the balanced equation.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":30,"explanation":"Reaction orders reflect how the rate of a reaction depends on the concentration of reactants. They are derived from rate laws, which are established through experiments. This distinction from stoichiometric coefficients highlights that reaction mechanisms can influence rates, leading to complex relationships not evident in balanced equations.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974930,"front":"How can the unit of k be calculated?","back":"The unit of k can be calculated by rearranging the rate equation, inserting the units, and simplifying the fraction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":31,"explanation":"The unit of the rate constant (k) is determined by analyzing the units of the rate equation components. By rearranging the equation to isolate k, plugging in the units of concentration and time, and simplifying, the unit of k can be derived. This process ensures dimensional consistency in the rate equation.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974933,"front":"Describe the concept of continuous monitoring in relation to rate of reaction.","back":"Continuous monitoring refers to following one experiment over time and recording the change in concentration. The gradient of the concentration-time graph represents the rate of reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":32,"explanation":"Continuous monitoring allows for real-time observation of reaction dynamics, providing insights into how concentration changes over time. This method enhances understanding of reaction kinetics, enabling the identification of factors affecting rates, such as temperature or catalysts, and facilitating more accurate modeling of chemical processes.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974937,"front":"What is the significance of having a large excess of reactants in a reaction?","back":"In reactions with several reactants, if one reactant is kept in a large excess, it will appear to have no effect on the rate and will be pseudo-zero order. This is because its concentration stays virtually constant and does not affect the rate.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":33,"explanation":"Having a large excess of a reactant in a reaction is significant because it essentially renders that reactant's concentration constant, making its impact on the reaction rate negligible. This allows for simplification of the reaction kinetics and can help in controlling the reaction outcome.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974940,"front":"What is a common clock reaction?","back":"A common clock reaction involves two successive reactions, where the end point is achieved when one limited reactant runs out, resulting in a sudden color change.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":34,"explanation":"Clock reactions are fascinating because they visually demonstrate reaction kinetics and the concept of reaction rates. The sudden color change serves as a clear indicator of the reaction's progress, making them popular in educational settings to illustrate chemical principles and the effects of concentration and temperature on reaction speed.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974941,"front":"How can the order of reaction be determined in a clock reaction?","back":"By repeating the experiment several times and varying the concentration of a reactant while keeping the other reactants at constant concentration, the order of reaction with respect to that reactant can be determined.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":35,"explanation":"In a clock reaction, the time taken for a color change to occur is measured. By altering the concentration of one reactant and observing the effect on the time taken for the color change, the order of reaction can be deduced. This method helps establish the relationship between reactant concentration and reaction rate.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974944,"front":"How can the of a reaction be calculated graphically?","back":"By plotting a graph of log rate vs log [Y], where Y is the concentration of one of the reactants that is changed, the gradient of the line obtained is equal to the order of the reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":38,"explanation":"Graphical methods provide a visual representation of the relationship between variables, making it easier to interpret data. The log-log plot is particularly useful in kinetics, as it linearizes the rate law, allowing for straightforward determination of reaction order through the slope, which reflects the sensitivity of the rate to concentration changes.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974945,"front":"Define the term 'order' in the context of a rate equation.","back":"The order of a reactant in a rate equation represents the power to which its concentration is raised in the rate equation.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":39,"explanation":"In rate equations, the order indicates how the rate of reaction is influenced by the concentration of reactants. A higher order suggests a more significant impact on the reaction rate, reflecting the complexity of molecular interactions and the reaction mechanism involved. Understanding order helps in predicting reaction behavior.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974946,"front":"What is the significance of high concentrations and quick times in experimental initial rate data?","back":"High concentrations and quick times in experiments can lead to the biggest percentage errors in the initial rate data.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":40,"explanation":"High concentrations and quick times in experimental initial rate data can introduce higher levels of variability and potential inaccuracies due to the increased likelihood of errors in measurements and reactions at such extreme conditions. This can impact the reliability and precision of the obtained initial rate data.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974947,"front":"Describe the effect of changing the concentration of both reactants simultaneously on the rate of a reaction.","back":"The effect of changing the concentration of both reactants simultaneously is that the individual changes in concentration are multiplied together to give an overall change in the rate of the reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":41,"explanation":"Changing the concentration of both reactants simultaneously affects the rate of the reaction by multiplying the individual concentration changes. This means that the overall impact on the reaction rate is a combined result of the changes in both reactant concentrations.","deleted_at":null,"flashcard_deck_id":"bLPnZ","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}}]

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