Hydrogen iodide decomposes to hydrogen and iodine by second order kinetics at 60

Question

Hydrogen iodide decomposes to hydrogen and iodine by second order kinetics at 600K with a rate constant of

9.7 x 10-6 M-1s-1.

If the initial concentration of HI is 0.100 M, calculate the molarity of HI after 6.0 days of reaction. Write the rate expression for this reaction

Hydrogen iodide decomposes to hydrogen and iodine by second order kinetics at 600K with a rate constant of 9.7 x 10^-6 M^-1 s^-1. 2H I (g) -- > H2 (g) +I 2 (g) If the initial concentration of HI is 0.100 M, calculate the molarity of HI after 6.0 days of reaction. Write the rate expression for this reaction

Explanation / Answer

1 / [A] = k t + 1 / [A]o

6 days = 518400 s

1/[A] = ( 9.7*10-6 * 518400 s ) + 1/0.1 = 15.03

[A] = 0.0665 M

k = [(1/[A]) - (1/[Ao])] / t

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