Question

The kinetics of a gas phase reaction of the form A → Products results in a rate constant of 1.308 M⁻¹ s⁻¹. For this reaction, the initial concentration of A is 0.155 M. What is the concentration of A after 0.385 seconds?

Answer 1

Answer:

$C_A=0.144M$

Explanation:

Hello,

In this case, given the rate constant, we infer this is about a second order reaction, whose equation is:

$\frac{dC_A}{dt}=kC_A^2$

Thus, by integration we obtain:

$\frac{1}{C_A}= \frac{1}{C_A_0}+kt$

Hence, we solve for the final concentration after 0.385 s:

$\frac{1}{C_A}= \frac{1}{0.155M}+\frac{1.308}{Ms} *0.385s=\frac{6.955}{M}\\ \\C_A=\frac{M}{6.955} \\\\C_A=0.144M$

Best regards.