At a certain temperature the rate of this reaction is first order in HI with a rate constant of :7.21s?1

2HI(g)??H2(g) + I2(g)

Suppose a vessel contains HI at a concentration of 0.440M

. Calculate the concentration of HI in the vessel 0.210 seconds later. You may assume no other reaction is important.

Round your answer to 2 significant digits.

The concentration of HI in the vessel after 0.210 seconds later will be 0.097 M.

Explanation:

Initial concentration of HI =

Final concentration after t seconds = [A]

t = 0.210 seconds

Rate constant of reaction = k =

The integrated rate law of first order kinetics :

[A] = 0.0968 M ≈ 0.097 M

The concentration of HI in the vessel after 0.210 seconds later will be 0.097 M.

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be