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

23.5

23.5

47.0

conduction is the transfer of thermal energy (heat in transfer) due to collisions between the molecules in the object. collisions between adjacent atoms and molecules transfer kinetic energy from the warmer to the cooler object. the objects must be in physical contact.