Integrated Rate Law

Question

The decomposition of nitrous oxide at 565 °C

N₂O(g)N₂(g) + ½ O₂(g)

is second order in N₂O with a rate constant of 1.10×10^-3 M^-1 s^-1.

If the initial concentration of N₂O is 1.67 M, the concentration of N₂O will be 0.391 M after ________seconds have passed.

Answer 1

The integrated rate law for a 2nd order reaction is...

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

Simply plug in the values for [A] = 0.391 M, [A]_o = 1.67 M, k = 1.10x10^-3 M^-1s^-1 and solve for t. Your answer will be in seconds.