At a certain temperature the rate of this reaction is first order in 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.

Complete question is;

Consider this reaction: 2 HI(g) ⇄ H₂(g) + I₂(g)

At a certain temperature, this reaction follows first - order kinetics with a rate constant of 0.684 s^(-1). Suppose a vessel contains HI at a concentration of 0.32 M. Calculate the concentration of HI in the vessel 0.88 seconds later.

You may assume no other reaction is important.

Round your answer to 2 significant digits

0.18 M

Explanation:

We are given;

Initial concentration of HI = 0.32 M

Time = 0.88 s

Rate is given as 0.684 s^(-1)

Now, we want to find the concentration of HI in the vessel 0.88 seconds later. It can be gotten from the formula;

ln (HI) = ln (HI)₀ - (kt)

Where;

(HI)₀ is the initial concentration

k is the reaction rate constant

t is time

Plugging in the relevant values, we have;

ln (HI) = In (0.32) - (0.684 × 0.88)

ln (HI) = -1.1394 - 0.6019

ln (HI) = -1.7413

(HI) = e^(-1.7413)

(HI) = 0.175 M ≈ 0.18 M