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

`C_A=0.144M`

Step-by-step explanation:

Hello,

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

`(dC_A)/(dt)=kC_A^2`

Thus, by integration we obtain:

`(1)/(C_A)= (1)/(C_A_0)+kt`

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

`(1)/(C_A)= (1)/(0.155M)+(1.308)/(Ms) *0.385s=(6.955)/(M)\\ \\C_A=(M)/(6.955) \\\\C_A=0.144M`

Best regards.