The gas phase decomposition of hydrogen iodide at 700 K HI(g)½ H2(g) + ½ I2(g) is second order in HI with a rate constant of 1.20×10-3 M-1 s-1. If the initial concentration of HI is 0.455 M, the concentration of HI will be 4.64×10-2 M after seconds have passed.

16130s

Explanation:

The integrated rate law for a second order reaction is given as;

1 / [A] = kt + 1 / [A]o

[A] = Final Concentration = 4.64×10-2 M

[A]o = Initial Concentration = 0.455 M

k = Rate constant = 1.20×10-3

t = ?

solving for t, we have;

kt = 1 / [A] - 1 / [A]o

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

t = [(1 / 4.64×10-2)  - (1 / 0.455)] / 1.20×10-3

t = (21.552 - 2.2) / 1.20×10-3

t = 16.13 ×10^3s =  16130s

explanation:

i think option no d is the correct answer