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Kinetics I (Worksheet)

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Work in groups on these problems. You should try to answer the questions without referring to your textbook. If you get stuck, try asking another group for help.

1. For the reaction below, if substance A is disappearing at a rate of \(1.82 \times 10^{–2} mol L^{-1}s^{-1}\), at what rate is C appearing?

\[3 A + 3 B \rightarrow 5 C + 2 D\]

 

 

 

 

 

2. Ozone (\(O_3\)) is produced in the stratosphere by the chemical reaction shown below. If at a given instant, molecular oxygen (\(O_2\)) is reacting at a rate of \(2.17 \times 10^{–5} mol L^{-1}s^{-1}\), at what rate is ozone being produced?

\[3 O2(g) \rightarrow 2 O3(g)\]

 

 

 

 


3. For the reaction,

\[H_2O_2(aq) + 3 I^−(aq) + 2 H^+(aq) \rightarrow 2 H_2O (l) + I_3^−(aq)\]

The rate law was experimentally determined to be

\[\text{Rate} =[H_2O_2][I^−]\]

  1. What is the reaction order in terms of \(H_2O_2\)?
  2. What is the reaction order in terms of \(I^−\)?
  3. What is the reaction order in terms of \(H^+\)?
  4. What is the overall reaction order of this reaction?
     

 

4. If a reaction is second order in \(B\) and the concentration of \(B\) increased from \(0.0850\, M\) to \(0.2975\, M\), what should happen to the rate?
 

 

5. The data below were collected for the reaction:

\[BrO_3^– + 5 Br^–+ H_3O^+ \rightarrow 3 Br_2+ 9 H_2O\]
 

Experiment # Initial Concentration of Reactants and Products (mol/L) Initial Rate (mol/L•s)
  \(BrO_3^–\) \(Br^–\) \(H_3O^+\) \(Br_2\)  
1 0.10 0.10 0.10 0 1.2
2 0.20 0.10 0.10 0 2.4
3 0.10 0.30 0.10 0 3.6
4 0.20 0.10 0.15 0 5.4
  1. Determine the rate law for this reaction.
  2. Calculate the value of \(k\) for this reaction and express it with the correct units.
  3. How would the Initial Rate change if the initial concentration of \(Br_2\) were to be non-zero?
     

 

 

 


6. The data below were collected for the reaction at 327 °C:

\[H_2(g) + I_2(g) \rightarrow 2 HI (g)\]

 

 

Experiment # Initial Concentration of Reactants and Products (M) Initial Rate (mol/L•s)
  \([H_2]\) \([I_2]\) \([HI]\)  
1 0.113 0.110 0 \(3.01 \times 10^{-4}\)
2 0.220 0.330 0 \(1.76 \times 10^{-3}\)
3 0.550 0.110 0 \(1.47 \times 10^{-3}\)
  1. Determine the rate law for this reaction.
  2. Calculate the value of \(k\) for this reaction and express it with the correct units.
  3. How would the Initial Rate change if the initial concentration of \(HI\) were to be non-zero?