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, here is the complete question:

At a certain temperature this reaction follows second-order kinetics with a rate constant of 14.1 M⁻¹s⁻¹

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

Suppose a vessel contains SO₃ at a concentration of 1.44 M. 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: The concentration of $SO_3$ in the vessel after 0.240 seconds is 0.24 M

Explanation:

For the given chemical equation:

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

The integrated rate law equation for second order reaction follows:

$k=\frac{1}{t}\left (\frac{1}{[A]}-\frac{1}{[A]_o}\right)$

where,

k = rate constant = $14.1M^{-1}s^{-1}$

t = time taken= 0.240 second

[A] = concentration of substance after time 't' = ?

$[A]_o$ = Initial concentration = 1.44 M

Putting values in above equation, we get:

$14.1=\frac{1}{0.240}\left (\frac{1}{[A]}-\frac{1}{1.44}\right)$

$[A]=0.245M$

Hence, the concentration of $SO_3$ in the vessel after 0.240 seconds is 0.24 M