Question

At a certain temperature this reaction follows second-order kinetics with a rate constant of : Suppose a vessel contains at a concentration of . Calculate the concentration of in the vessel seconds later. You may assume no other reaction is important. Round your answer to significant digits.

Answer 1

The question is incomplete, the complete question is:

At a certain temperature this reaction follows second-order kinetics with a rate constant of 14.1$M^{-1}s^{-1}$ :

$2SO_3(g)\rightarrow 2SO_2(g)+O_2(g)$

Suppose a vessel contains $SO_3$ at a concentration of 1.44 M . Calculate the concentration of

Answer:

The concentration of $SO_3$ in the vessel 0.240 seconds later will be 0.2452 M.

Explanation:

Integrated rate law for second order kinetics is given by:

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

k = rate constant

$a_0$ = initial concentration

a = Concentration after time t.

We have :

$2SO_3(g)\rightarrow 2SO_2(g)+O_2(g)$

Initial concentration $SO_3$ = $a_0=1.44 M$

Final concentration $SO_3$ at t = a =?

t = 0.240 s

Rate constant of the reaction = k = 14.1$M^{-1}s^{-1}$

$\frac{1}{a}=14.1 M^{-1}s^{-1}\times 0.240 s+\frac{1}{1.44 M}$

$a=0.2452 M$

The concentration of $SO_3$ in the vessel 0.240 seconds later will be 0.2452 M.