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.

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

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.

The concentration of in the vessel after 0.240 seconds is 0.24 M

Explanation:

For the given chemical equation:

The integrated rate law equation for second order reaction follows:

where,

k = rate constant =

t = time taken= 0.240 second

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

= Initial concentration = 1.44 M

Putting values in above equation, we get:

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

the answer is true.

false

because it does not have the potential to be entirely used up