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

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


We're given the following rate law:

rate=kNH2NO


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

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