Question

"The rate law for the reaction NH2 (g) + NO (g) → N2 (g) + H2O (g) was determined to be as follows: Rate = k[NH2][NO]. In an experiment at 1200K, where the initial concentration of NH2 was 1.00 × 10−5 M and the initial concentration of NO was 1.00 × 10−5 M, the reaction rate was measured to be 0.12 M/s. Calculate the value of the rate constant."

Answer 1

Value of rate constant is
`1.2* 10^(9)M^(-1)s^(-1)`

Step-by-step explanation:

`Rate=k[NH_(2)][NO]`

Here k is the rate constant of the reaction.

species inside third bracket represents concentration.

Rate constant only depends upon temperature and not on the progress of a reaction.

Here initial concentration of
`NH_(2)` =
`1.00* 10^(-5)M`

initial concentration of NO =
`1.00* 10^(-5)M`

Inital rate of reaction = 0.12 M/s

So,
`k=(Rate of reaction)/([NH_(2)][NO])=(0.12)/((1.00* 10^(-5))^(2))M^(-1)s^(-1)=1.2* 10^(9)M^(-1)s^(-1)`