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Kinetics

A-Level AQA Chemistry

This pack of flashcards covers key concepts of reaction kinetics and collision theory, including definitions of activation energy, the Maxwell-Boltzmann distribution, factors affecting reaction rates like temperature, concentration, surface area, and the role of catalysts. It explains how these factors influence the energy of particles, collision frequency, and effective collisions, contributing to the rate of chemical reactions.

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"Describe the collision theory."	"Reactions can only occur when collisions take place between particles having sufficient energy."
"Define activation energy."	"The minimum energy which particles need to collide to start a reaction."
"What does the Maxwell-Boltzmann energy distribution show?"	"The spread of energies that molecules of a gas or liquid have at a particular temperature."
"How can a reaction go to completion if few particles have energy greater than EA?"	"Particles can gain energy through collisions."
"What happens to the energy distribution as temperature increases?"	"The distribution shifts towards having more molecules with higher energies."
"What happens to the Emp and mean energy as temperature increases?"	"Both the Emp and mean energy shift to higher energy values."
"What happens to the number of molecules with higher energies as temperature decreases?"	"The number of molecules with higher energies decreases."
"What happens to the energy distribution at higher temperatures compared to lower temperatures?"	"At higher temperatures, the molecules have a wider range of energies than at lower temperatures."
"What is the rate of reaction defined as?"	"The rate of reaction is defined as the change in concentration of a substance in unit time."
"How is the rate of reaction usually measured?"	"The rate of reaction is usually measured in mol."
"Describe how the rate of reaction can be determined from a graph."	"The rate of reaction can be determined from a graph by calculating the gradient of the curve."
"What is the initial rate of reaction?"	"The initial rate of reaction is the rate at the start of the reaction where it is fastest."
"How can reaction rates be calculated from concentration graphs?"	"Reaction rates can be calculated from concentration graphs by drawing tangents to the curve at different times and calculating the gradient of the tangent."
"What is the effect of increasing concentration on collision frequency?"	"Increasing concentration leads to a higher frequency of effective collisions due to more particles per unit volume."
"What happens to the shape of energy distribution curves when concentration increases?"	"The shape of energy distribution curves does not change when concentration increases."
"What is the relationship between concentration and the area under energy distribution curves?"	"The area under energy distribution curves increases with higher concentration because there are more particles."
"What determines the rate of reaction?"	"The rate of reaction is determined by factors such as concentration, temperature, and surface area."
"Describe the effect of increasing temperature on the rate of a reaction."	"At higher temperatures, the energy of the particles increases, resulting in more frequent collisions with energy greater than the activation energy, leading to an increase in the rate of the reaction."
"What is the effect of increasing surface area on the rate of a reaction?"	"Increasing surface area causes successful collisions to occur more frequently between the reactant particles, resulting in an increase in the rate of the reaction."
"Define catalysts."	"Catalysts are substances that increase reaction rates without getting used up."
"How do catalysts increase reaction rates?"	"Catalysts provide an alternative route or mechanism with a lower activation energy, allowing more particles to have energy greater than the activation energy and increasing the frequency of effective collisions."
"Compare the activation energies for an uncatalyzed reaction and the same reaction with a catalyst present."	"The activation energy for the reaction with a catalyst present is lower compared to the uncatalyzed reaction."
"Describe the progress of a reaction with a lower activation energy."	"With a lower activation energy, more particles will have energy greater than the activation energy, resulting in a higher frequency of effective collisions and a faster reaction rate."

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Describe the collision theory.

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Reactions can only occur when collisions take place between particles having sufficient energy.

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[{"id":974785,"front":"Describe the collision theory.","back":"Reactions can only occur when collisions take place between particles having sufficient energy.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The collision theory explains that for a chemical reaction to occur, particles must collide with each other. However, not all collisions lead to a reaction. Only collisions between particles with enough energy, known as activation energy, can result in a successful reaction. This theory helps us understand the factors that influence reaction rates, such as temperature and concentration, as they affect the frequency and energy of collisions.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974786,"front":"Define activation energy.","back":"The minimum energy which particles need to collide to start a reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Activation energy is a crucial concept in chemistry. It represents the minimum amount of energy required for a chemical reaction to occur. This energy is necessary to overcome the energy barrier between reactants and products. Without sufficient activation energy, particles will not have enough energy to collide and initiate the reaction. In other words, activation energy determines the rate at which a reaction proceeds.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974787,"front":"What does the Maxwell-Boltzmann energy distribution show?","back":"The spread of energies that molecules of a gas or liquid have at a particular temperature.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The Maxwell-Boltzmann energy distribution is a statistical model that describes the distribution of energies among molecules in a gas or liquid at a given temperature. It shows that molecules have a range of energies, with some having higher energies and others having lower energies. This distribution is important in understanding various properties of gases and liquids, such as their heat capacity and the likelihood of certain reactions occurring.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974789,"front":"How can a reaction go to completion if few particles have energy greater than EA?","back":"Particles can gain energy through collisions.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"In a reaction, particles need to overcome the activation energy (EA) barrier to proceed. Even if only a few particles initially have enough energy, collisions between particles can transfer energy, allowing more particles to reach the required energy level. This energy transfer through collisions increases the likelihood of particles surpassing EA and the reaction proceeding to completion.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974790,"front":"What happens to the energy distribution as temperature increases?","back":"The distribution shifts towards having more molecules with higher energies.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"As temperature increases, the average kinetic energy of molecules rises, leading to a greater proportion of molecules with higher energies. This is due to the increased thermal motion and collisions, causing more molecules to attain higher energy states.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974792,"front":"What happens to the Emp and mean energy as temperature increases?","back":"Both the Emp and mean energy shift to higher energy values.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"As temperature increases, the Emp (most probable energy) and mean energy of a system also increase. This is because at higher temperatures, particles in the system have more kinetic energy and move faster. As a result, the distribution of energies shifts towards higher values, leading to an increase in both the Emp and mean energy.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974794,"front":"What happens to the number of molecules with higher energies as temperature decreases?","back":"The number of molecules with higher energies decreases.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"As temperature decreases, the average kinetic energy of molecules decreases. This means that fewer molecules have enough energy to reach higher energy states. Therefore, the number of molecules with higher energies decreases as temperature decreases.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974795,"front":"What happens to the energy distribution at higher temperatures compared to lower temperatures?","back":"At higher temperatures, the molecules have a wider range of energies than at lower temperatures.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"At higher temperatures, molecules have more kinetic energy, leading to a wider distribution of energy levels. This is due to increased molecular motion and collisions, resulting in a broader range of energy states. Conversely, at lower temperatures, molecules have less kinetic energy and a narrower distribution of energy levels.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974797,"front":"What is the rate of reaction defined as?","back":"The rate of reaction is defined as the change in concentration of a substance in unit time.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The rate of reaction is defined as the change in concentration of a substance per unit time. This definition is fundamental in understanding how quickly reactants are consumed or products are formed in a chemical reaction. It provides a quantitative measure of reaction speed.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974799,"front":"How is the rate of reaction usually measured?","back":"The rate of reaction is usually measured in mol.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The rate of reaction is typically measured in terms of the change in the amount of reactants or products over time. This is commonly expressed in units of moles, as it allows for a quantitative measurement of the progress of the reaction. By tracking the change in the number of moles of a substance involved in the reaction, scientists can determine the rate at which the reaction is occurring.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974800,"front":"Describe how the rate of reaction can be determined from a graph.","back":"The rate of reaction can be determined from a graph by calculating the gradient of the curve.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Calculating the gradient of a curve on a graph allows for the determination of the rate of reaction. This is because the gradient represents the rate of change at any given point on the graph. By analyzing the slope, one can ascertain the rate at which the reaction is progressing.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974802,"front":"What is the initial rate of reaction?","back":"The initial rate of reaction is the rate at the start of the reaction where it is fastest.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The initial rate of reaction is a measure of how quickly a reaction proceeds at the very beginning, when the reactants are first mixed. It is typically the fastest rate observed during the reaction. This rate provides important information about the reaction mechanism and the concentration of reactants. By determining the initial rate, scientists can gain insights into the factors that affect the reaction and make predictions about its behavior over time.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974803,"front":"How can reaction rates be calculated from concentration graphs?","back":"Reaction rates can be calculated from concentration graphs by drawing tangents to the curve at different times and calculating the gradient of the tangent.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Reaction rates can be calculated from concentration graphs by determining the slope of the tangent line at different points on the curve. The tangent line represents the instantaneous rate of change at that specific time. By calculating the gradient of the tangent, which is the change in concentration divided by the change in time, the reaction rate can be determined. This method allows for the determination of the rate of reaction at any given time during the reaction.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974807,"front":"What is the effect of increasing concentration on collision frequency?","back":"Increasing concentration leads to a higher frequency of effective collisions due to more particles per unit volume.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Increasing the concentration of a substance means there are more particles in the same volume. This results in a higher likelihood of these particles colliding with each other, leading to an increased frequency of effective collisions. This is due to the increased chances of successful interactions between the reacting species.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974808,"front":"What happens to the shape of energy distribution curves when concentration increases?","back":"The shape of energy distribution curves does not change when concentration increases.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"When concentration increases, the shape of energy distribution curves remains the same. This is because concentration only affects the number of particles present, not their energy distribution. The shape of the curve is determined by the energy levels of the particles, which are independent of concentration. Therefore, increasing concentration does not alter the shape of the energy distribution curve.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974809,"front":"What is the relationship between concentration and the area under energy distribution curves?","back":"The area under energy distribution curves increases with higher concentration because there are more particles.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The relationship between concentration and the area under energy distribution curves is influenced by the number of particles present. Higher concentration means more particles, leading to an increase in the area under the energy distribution curve. This is due to the greater number of particles contributing to the overall energy distribution.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974811,"front":"What determines the rate of reaction?","back":"The rate of reaction is determined by factors such as concentration, temperature, and surface area.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The rate of a chemical reaction is influenced by several factors. Concentration affects the frequency of collisions between reactant molecules, while temperature impacts the kinetic energy of the molecules. Additionally, surface area affects the frequency of collisions in heterogeneous reactions.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974813,"front":"Describe the effect of increasing temperature on the rate of a reaction.","back":"At higher temperatures, the energy of the particles increases, resulting in more frequent collisions with energy greater than the activation energy, leading to an increase in the rate of the reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Increasing temperature provides more kinetic energy to the particles involved in a reaction. This leads to a higher frequency of collisions and a greater proportion of collisions with sufficient energy to overcome the activation energy barrier. Consequently, the reaction rate increases as a result of these more energetic collisions.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974815,"front":"What is the effect of increasing surface area on the rate of a reaction?","back":"Increasing surface area causes successful collisions to occur more frequently between the reactant particles, resulting in an increase in the rate of the reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Increasing the surface area of a reactant increases the number of exposed particles available for collisions. This leads to a higher frequency of successful collisions between reactant particles, which in turn increases the rate of the reaction. This is because a larger surface area provides more opportunities for reactant particles to come into contact with each other, leading to a faster reaction.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974816,"front":"Define catalysts.","back":"Catalysts are substances that increase reaction rates without getting used up.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Catalysts work by providing an alternative reaction pathway with lower activation energy, allowing the reaction to occur more readily. This enables them to speed up chemical reactions without being consumed in the process, making them highly efficient in industrial and biological processes.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974817,"front":"How do catalysts increase reaction rates?","back":"Catalysts provide an alternative route or mechanism with a lower activation energy, allowing more particles to have energy greater than the activation energy and increasing the frequency of effective collisions.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Catalysts increase reaction rates by lowering the activation energy required for a reaction to occur. This allows more particles to have sufficient energy to overcome the activation energy barrier, leading to an increase in the frequency of effective collisions. By providing an alternative reaction pathway, catalysts facilitate the formation of products more quickly, without being consumed in the process.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974818,"front":"Compare the activation energies for an uncatalyzed reaction and the same reaction with a catalyst present.","back":"The activation energy for the reaction with a catalyst present is lower compared to the uncatalyzed reaction.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The presence of a catalyst lowers the activation energy for a reaction. This is because a catalyst provides an alternative reaction pathway with a lower energy barrier. By lowering the activation energy, a catalyst increases the rate of the reaction without being consumed in the process. This is why catalysts are often used in industrial processes to increase reaction rates and efficiency.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974819,"front":"Describe the progress of a reaction with a lower activation energy.","back":"With a lower activation energy, more particles will have energy greater than the activation energy, resulting in a higher frequency of effective collisions and a faster reaction rate.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"A reaction with a lower activation energy allows more particles to have sufficient energy to overcome the energy barrier and react. This leads to an increase in the frequency of successful collisions between reactant particles, resulting in a faster reaction rate. Lowering the activation energy can be achieved by using catalysts or increasing the temperature, both of which provide more energy to the reacting particles.","deleted_at":null,"flashcard_deck_id":"AMcyw","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}}]

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