# Kinetics Solutions

- Page ID
- 11041

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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 Write the rate expression in terms of D[reactant]/Dt and D[product]/Dt:

rate = - D[N_{2}]/Dt = - D[H_{2}]/3Dt = D[NH_{3}]/2Dt

2 Determine

- a) the order of each reactant: 1st order in A; zero order in B
- b) the order of the reaction: overall reaction is 1st ordered
- c) write the rate law: rate = k[A]
- d) calculate the rate constant, k: k = 1.75 x 10
^{-2}/s

3a. The decomposition of A_{2}B_{3} is second order with a k = 6.5 x 10^{-5} M^{-1}s^{ -1} at 25^{o}C. If the initial concentration is 0.50 M, the concentration after 3 min is: 0.497 M

b. The half-life for the reaction in question 3a is: 3.08 x 10^{4} s

4. The decomposition of AB is first order with a k = 2.3 x 10^{-7} s^{-1} at 45^{o}C. If the initial concentration is 0.25 M, the concentration after 2.3 min is: 0.25 M

b. The half-life for the reaction in question 4a is: 3.01 x 10^{6} s

5a. The concentration of reactant after 2.5 minutes if the inital concentration was 0.100 M and k = 6.93 x 10^{-3 }s^{-1} for a first order reaction is: 0.0354 M

b. The half-life is: 100 s

6. For the first order reaction:

\[SO_2Cl_2 \rightarrow SO_2 + Cl_2\]

How long will it take to reach 0.31 x 10^{-3} M if the inital concentration was 1.25 x 10^{-3} M and k = 0.17/hr? 8.2 hrs

7. For the second order reaction \(A \rightarrow B\) (k = 1.5 x 10^{-2}/Ms),

- if the initial concentration of A is 0.10M, the concentration of A after 4 min is: 0.074 M
- the half-life is: 667 s