# Problem: 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 1200 K, 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.a. 1.2 × 10−11 M−1s−1b. 1.2 × 109 M−1sc. 1.2 × 109 s−1d. 1.2 × 109 M−1s−1

###### FREE Expert Solution

We’re being asked to calculate the rate constant the value of the rate constant.

We're given the following rate law:

$\overline{){\mathbf{rate}}{\mathbf{=}}{\mathbf{k}}\left[{\mathbf{NH}}_{\mathbf{2}}\right]\left[\mathbf{NO}\right]}$

Given:

[NH2] = 1.00×10−5 M
[NO] = 1.00×10−5 M
rate = 0.12 M/s

Calculate the rate constant, k:

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###### Problem Details

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 1200 K, 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.

a. 1.2 × 10−11 M−1s−1

b. 1.2 × 109 M−1s

c. 1.2 × 109 s−1

d. 1.2 × 109 M−1s−1

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Rate Law concept. You can view video lessons to learn Rate Law. Or if you need more Rate Law practice, you can also practice Rate Law practice problems.