The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of

ID: 483082 • Letter: T

Question

The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.44×104 s1at a certain temperature.

The half-life for this reaction is:

Part B

How long will it take for the concentration of SO2Cl2 to decrease to 25% of its initial concentration? (answer in seconds please)

Part C

If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.76 M ?

Part D

If the initial concentration of SO2Cl2 is 0.175 M , what is the concentration of SO2Cl2 after 190 s ?

Part E

If the initial concentration of SO2Cl2 is 0.175 M , what is the concentration of SO2Cl2 after 510 s ?

t1/2 = 4810 s

A)
for 1st order reaction
half life = ln 2/ k
= 0.693/k
= 0.693 / (1.44*10^-4)
= 4812.5 s
Answer: 4810 s

B)
concentration will decrease to 25% is 2 half lifes
hence time taken = 2*4812.5 = 9625 s
Answer: 9620 s

C)
use:
[A] = [A]o*e^(-k*t)
0.76 = 1.00 *e^(-1.44*10^-4 *t)
1.44*10^-4 *t = 0.2744
t = 1906 s
Answer: 1910 s

D)
[A] = [A]o*e^(-k*t)
[A] = 0.175 *e^(-1.44*10^-4 *190)
[A] = 0.175*0.973
= 0.17 M
Answer: 0.17 M

E)
[A] = [A]o*e^(-k*t)
[A] = 0.175 *e^(-1.44*10^-4 *510)
[A] = 0.175*0.9292
= 0.163 M
Answer: 0.163 M

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