In this worksheet, we will practice calculating reaction rates using variables such as concentration, pressure, conductivity, and optical absorption.

**Q1: **

Ammonia decomposes into hydrogen and nitrogen at high temperature. The rate of decomposition of ammonia is found to be M/s.

Write a balanced chemical equation for this reaction.

- A
- B
- C
- D
- E

What is the rate of formation of nitrogen?

- A M/s
- B M/s
- C M/s
- D M/s
- E M/s

What is the rate of formation of hydrogen?

- A M/s
- B M/s
- C M/s
- D M/s
- E M/s

**Q2: **

Aqueous hydrogen peroxide () decomposes into oxygen and water. The rate of decomposition of hydrogen peroxide is found to be M/h.

Write a balanced chemical equation for this reaction.

- A
- B
- C
- D
- E

What is the rate of formation of water?

- A M/h
- B M/h
- C M/h
- D M/h
- E M/h

What is the rate of formation of oxygen?

- A M/h
- B M/h
- C M/h
- D M/h
- E M/h

**Q3: **

The equilibrium for the ionization of the ion, a weak acid used in some household cleaners, is shown. For a mixture of and at equilibrium, the following are the concentrations:

= 0.027 M,

= 0.29 M,

= 0.13 M.

What is the equilibrium constant for this reaction under these conditions?

- A M/s
- B M/s
- C M/s
- D M/s
- E M/s

**Q4: **

Dinitrogen pentoxide decomposes in chloroform to form nitrogen dioxide and oxygen, as shown. The decomposition is a first-order reaction with a rate constant of min^{−1} at . Calculate the rate of reaction in molarity per second when [] = 0.400 M.

- A M/s
- B M/s
- C M/s
- D M/s
- E M/s

**Q5: **

A reaction begins at a time = 0 and is monitored over a period of time, , by measuring the reactant concentration, , at fixed time intervals. How is the average rate of reaction for this time period calculated from a graph of against ?

- ABy calculating the total area under the graph between = 0 and =
- BBy fitting a polynomial function to the curve and evaluating the derivative of this function at =
- CBy calculating the gradient of the tangent at =
- DBy dividing the change in between = 0 and = by
- EBy calculating the gradient of the tangent at =

**Q6: **

A reaction begins at a time = 0 and is monitored over a period of time, , by measuring the reactant concentration, , at fixed time intervals. How is the instantaneous rate at calculated from a graph of against ?

- ABy calculating the total area under the graph between = 0 and =
- BBy fitting a polynomial function to the curve and evaluating the derivative of this function at =
- CBy dividing the change in between = 0 and = by
- DBy calculating the gradient of the tangent at =
- EBy calculating the gradient of the tangent at =