Question

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 M. What is the rate constant for this reaction?4.5 × 10-2 M-1s-11.0 × 10-2 M-1s-12.2 × 10-2 M-1s-13.8 × 10-2 M-1s-19.7 × 10-2 M-1s-1

Answer 1

Answer:
`9.7* 10^(-2)M^(-1)s^(-1)`

Step-by-step explanation:

Half life is the amount of time taken by a radioactive material to decay to half of its original value.

Half life for second order kinetics is given by:

`t_{(1)/(2)=(1)/(k* a_0)`

`t_{(1)/(2)` = half life = 15.4 s

k = rate constant =?

`a_0` = initial concentration = 0.67

`15.4s=(1)/(k* 0.67M)`

`k=9.7* 10^(-2)M^(-1)s^(-1)`

Thus the rate constant for this reaction is
`9.7* 10^(-2)M^(-1)s^(-1)`