IB Chemistry Kinetics Exam Questions and Answers

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Kinetics Review Questions

  1. Define rate of reaction 
  2. What are the units of the rate of reaction?
  3. Outline procedures by which you could obtain a value for the rate of reaction
  4. Draw a graph that shows the concentration of products with time as a reaction goes to completion. Explain the shape of the graph.
  5. Draw a graph that shows the concentration of reactants with time as a reaction goes to completion. Explain the shape of the graph.
  6. Outline the main features of collision theory
  7. Give two reasons why a collision would not result in a reaction
  8. The reaction between nitrogen and oxygen in the atmosphere under normal conditions is extremely slow. Which statement best explains this?
  1. The concentration of oxygen is much lower than that of nitrogen
  2. The molar mass of nitrogen is less than that of oxygen
  3. The frequency of collisions between nitrogen and oxygen molecules is lower than that between nitrogen molecules themselves
  4. Very few nitrogen and oxygen molecules have sufficient energy to react
  1. List 4 factors that affect reaction rates and explain why using the principles of collision theory.
  2. Define activation energy 
  3. Sketch a Maxwell-Boltzmann Energy Distribution Curve for two different temperatures.  
  4. Does activation energy change with temperature?
  5. How does the number of molecules with the required activation energy change at higher temperatures? Use energy distribution to explain.
  6. Give two reasons why a temperature increase, increases reaction rate and identify the more important reason.
  7. Will the following changes increase the reaction rate of the following reaction when 50 cm3 of 1.0 mol dm-3 HCl is added to 1.0 g calcium carbonate?

CaCO3(s) + 2 HCl (aq) → CaCl2 + CO2(g) + H2O(l)

  1. increasing volume of HCl
  2. increasing mass of CaCO3
  3. decreasing size of CaCO3 particles
  4. decreasing amount of CO2 present
  5. increasing temperature
  6. adding water to the reaction
  7. removing water from the reaction vessel
  8. adding a catalyst
  1. Explain, using the Maxwell-Boltzmann Energy distribution, why adding a catalyst increases reaction rate.
  2.  Determine the rate law for the following reaction

A + 2B →  AB2

  1. Using the data from the previous problem, calculate the rate constant
  2. What would the rate be if the [A] = 2.5 mol dm-3 and [B] = 3.0 mol dm-3?
  3. Determine the rate law for the following reaction

C2 + 2 D → 2 CD

  1. Using the data from the previous problem, calculate the rate constant
  2. What would the rate be if the [C] = 0.25 mol dm-3 and [D] = 0.30 mol dm-3?

  1. What is the order of reaction for the following rate laws

  1. Give the integrated rate law, the t1/2 equation, and the plot that would give a straight line for the following:

  1. A plot of ln [NO] vs time gives a straight line.
  1. Sketch the graph
  2. Write the rate law
  3. What is the molecularity of this reaction?
  1. A plot of [N2] vs time gives a straight line.
  1. Sketch the graph
  2. Write the rate law
  3. What is the molecularity of this reaction?
  1. Given the graph below,

  1. Give the rate law
  2. Calculate the rate constant
  3. Determine the half-life in the initial concentration of [A] is 2.0 mol dm-3
  4. What is the molecularity of this reaction?
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  1. Define half-life
  2. Given the graph to the right, determine the half-life of the reaction:  A + B → AB

  1. Define activated complex
  2. Give two examples of possible activated complexes that could be formed in the following reaction.

CH3Br  + OH-1 → CH3OH + Br-1

  1. Describe, in terms of bonds breaking and forming, two ways that the above reaction could occur.
  2. Draw an energy diagram for the above reaction.  Assume the reaction is exothermic.
  3. Show on your diagram, what happens when a catalyst is ...

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