Question

At a certain temperature this reaction follows second-order kinetics with a rate constant of 14.1·M−1s−1 : →2SO3g+2SO2gO2g Suppose a vessel contains SO3 at a concentration of 1.44M . Calculate the concentration of SO3 in the vessel 0.240 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

Answer 1

`[SO_3]=0.25M`

Step-by-step explanation:

Hello there!

In this case, since the integrated rate law for a second-order reaction is:

`[SO_3]=([SO_3]_0)/(1+kt[SO_3]_0)`

Thus, we plug in the initial concentration, rate constant and elapsed time to obtain:

`[SO_3]=(1.44M)/(1+14.1M^(-1)s^(-1)*0.240s*1.44M)\\\\`

`[SO_3]=0.25M`

Best regards!