Question

The reaction X → products is second order in X and has a rate constant of 0.035 M−1s−1. If a reaction mixture is initially 0.45 M in X, what is the concentration of X after 155 seconds?

Answer 1

Answer: The concentration of X after 155 seconds is 0.13 M

Explanation:

$X\rightarrow products$

$rate=k[X]^2$

Integrated rate law for second order kinetics is given by:

$\frac{1}{a}=kt+\frac{1}{a_0}$

$a_o$ = initial concentration = 0.45 M

a= concentration left after time t = ?

k = rate constant = $0.035M^{-1}s^{-1}$

t = time of decmposition = 155 s

$\frac{1}{a}=0.035\times 155+\frac{1}{0.45}$

$a=0.13M$

Thus the concentration of X after 155 seconds is 0.13 M

Answer 2

Answer:

0.13 M

Explanation: