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Questions and Answers
What does the average rate of a reaction depend on?
What are the units of the rate of a reaction when concentration is expressed in mol L–1 and time in seconds?
When calculating the average rate of a reaction, what mathematical operation is used with the changes in concentration and time?
In gaseous reactions, how is the concentration expressed to determine the rate of reaction?
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What is the average rate of a reaction if the change in concentration of a reactant over 100 seconds is 0.010 mol L–1?
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What does the rate constant depend on according to the Arrhenius equation?
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What is the order of a reaction with respect to a reactant determined by?
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What does the slope of the plot of ln k vs 1/T represent?
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Which statement about molecularity is correct?
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What happens to the rate of a reaction when the temperature increases by 10K?
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When subtracting equation (3.20) from equation (3.21), what do you obtain?
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How is the average rate of a reaction defined?
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What remains constant for a given reaction in the provided equations?
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At higher temperatures, what is expected to happen to the rate constant based on the Arrhenius equation?
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In the example provided, what is the value of k1 at 500K?
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Which of the following does not affect the rate of a chemical reaction?
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Which equation correctly relates k1 and k2 using the temperature terms?
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In a reaction, what is the relationship between rate constant and activation energy?
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What is the significance of the term 'threshold energy' in a chemical reaction?
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What does decreasing the activation energy result in according to the Arrhenius equation?
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For the reaction 2HI(g) → H2(g) + I2(g), how is the rate of the reaction expressed?
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What does the parameter Ea represent in the context of chemical reactions?
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How does the presence of a catalyst affect the activation energy in a chemical reaction?
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In the modified Arrhenius equation, what does the steric factor P account for?
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Given the rate expression rate = k[NO]², what is the order of the reaction with respect to NO?
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What is the unit of the rate constant k for a reaction where the rate is given as mol L⁻¹ s⁻¹ and the reaction is second order?
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When [A] is 0.1 mol L⁻¹ and [B] is 0.2 mol L⁻¹ in the reaction 2A + B → A2B, what is the initial rate of the reaction if k = 2.0 × 10⁻⁶ mol⁻² L² s⁻¹?
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What is the instantaneous rate of hydrolysis of butyl chloride at t = 600 s?
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Which term in the equation ln k = -Ea/(RT) + ln A represents the constant factor for the reaction?
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In the reaction Hg(l) + Cl2(g) → HgCl2(s), what can be said about the rates of the reactants and products?
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What is represented by the variable rinst in the context of chemical reactions?
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When two moles of a reactant decompose to form products in a reaction, what must be considered to express the rate correctly?
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If the instantaneous rate of HI decomposition is at a certain moment, what must be true regarding H2 and I2?
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At what concentration does the instantaneous rate of butyl chloride hydrolysis equal $1.0 \times 10^{-4}$ mol L$^{-1}$ s$^{-1}$?
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What is the significance of the pre-exponential factor A in the Arrhenius equation?
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How can the instantaneous rate be determined graphically for a reaction?
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In a zero order reaction involving the decomposition of NH3, what remains constant regardless of the concentration of reactants?
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Study Notes
Rate of a Reaction
- The rate of a reaction can be defined as the change in concentration of reactants or products per unit time.
- The average rate is calculated over a large interval of time, while the instantaneous rate is calculated at a specific moment in time.
- The units for the rate of a reaction are concentration time–1. For instance, if the concentration is in mol L–1 and time is in seconds, the units would be mol L–1s–1.
- When dealing with gaseous reactions and the concentration of gases is expressed in terms of partial pressures, the units of the rate equation will be atm s–1.
Factors Affecting Rate of a Reaction
- Temperature: Increasing temperature generally leads to a faster reaction rate.
- Concentration of Reactants: Greater concentration of reactants typically results in a faster reaction rate.
- Catalyst: Catalysts speed up a reaction without being consumed themselves.
- Surface Area: For reactions involving solids, increasing surface area usually leads to an increased reaction rate.
Rate Law
- The mathematical representation of the rate of a reaction is given by the rate law.
- The rate law is an experimentally determined equation that shows how the rate of a reaction depends on the concentrations of the reactants.
- It cannot be predicted theoretically.
Order of a Reaction
- The order of a reaction with respect to a reactant is the power of that reactant's concentration in the rate law equation.
- The overall order of a reaction is the sum of the orders with respect to each reactant.
Rate Constant
- The rate constant, denoted by 'k', is a proportionality factor in the rate law.
- It represents the rate of the reaction when the concentrations of all reactants are 1.
- The rate constant is a specific value for a given reaction at a given temperature.
Molecularity
- Molecularity refers to the number of molecules that participate in an elementary reaction step.
- It is only defined for elementary reactions, which are the individual steps of a complex reaction.
- The values of molecularity are usually limited to 1, 2, or 3, corresponding to unimolecular, bimolecular, and termolecular reactions, respectively.
Arrhenius Equation
- The Arrhenius equation describes the temperature dependence of the rate constant.
- k = Ae–Ea/RT
- k: Rate constant
- A: Arrhenius factor (pre-exponential factor)
- Ea: Activation energy
- R: Gas constant
- T: Temperature
- The equation shows that increasing temperature or decreasing the activation energy leads to an increase in the reaction rate and an exponential increase in the rate constant.
Collision Theory
- Collision theory suggests that for a reaction to occur, reactant molecules must collide with sufficient energy and proper orientation.
- The activation energy (Ea) is the minimum energy required for a collision to be effective.
- The frequency of collisions is influenced by factors such as temperature and concentration.
- The steric factor (P) accounts for the probability of collisions having the correct orientation for a reaction.
- The Arrhenius equation is modified to incorporate the steric factor: k P Z ABe E a / RT
Threshold Energy
- Threshold energy is the minimum energy required for a reaction to occur.
- It is the sum of the activation energy and the energy possessed by the reacting species.
Instantaneous Rate
- Instantaneous rate is determined at a specific moment in time and can be determined by drawing a tangent to the concentration vs. time curve at that point.
- The slope of the tangent represents the instantaneous rate.
Summary
- Chemical kinetics is the area of chemistry that studies reaction rates and the factors that influence them.
- Key factors influencing reaction rates include temperature, concentration, catalysts, and surface area.
- The rate law expresses the mathematical relationship between the rate and reactant concentrations.
- The order of a reaction describes how changes in reactant concentration affect the rate.
- The rate constant reflects the specific rate of a reaction under given conditions.
- Molecularity refers to the number of molecules involved in an elementary reaction step.
- The Arrhenius equation relates the rate constant to temperature and activation energy.
- Collision theory explains the basis for the energy requirement of reactions.
- The threshold energy is the minimum energy needed for a reaction to occur and is the sum of the activation energy and the energy of the reactant molecules.
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Description
Test your understanding of the rate of reactions, including factors that affect it such as temperature, concentration, catalysts, and surface area. This quiz will challenge your knowledge of both average and instantaneous rates of reactions in chemistry. Perfect for students studying chemical kinetics!