Question

What would happen to the rate of a reaction with rate law rate = `k[NO]^2[H_2]` if the concentration of `NO` were doubled?

Answer 1

The rate would quadruple.

Explanation:

`"Rate 1"` `=` `k[NO]^2[H_2]`

`"Rate 2"` `=` `k[2NO]^2[H_2]` `=` `"Rate 2"` `=` `4k[NO]^2[H_2]`

`"Rate 2"/"Rate 1"` `=` `[4k[NO]^2[H_2]]/[k[NO]^2[H_2]]` `=` `4`