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"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."

Respuesta :

JannetPalos

Answer:

Value of rate constant is [tex]1.2\times 10^{9}M^{-1}s^{-1}[/tex]

Explanation:

[tex]Rate=k[NH_{2}][NO][/tex]

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 [tex]NH_{2}[/tex] = [tex]1.00\times 10^{-5}M[/tex]

initial concentration of NO = [tex]1.00\times 10^{-5}M[/tex]

Inital rate of reaction = 0.12 M/s

So, [tex]k=\frac{Rate of reaction}{[NH_{2}][NO]}=\frac{0.12}{(1.00\times 10^{-5})^{2}}M^{-1}s^{-1}=1.2\times 10^{9}M^{-1}s^{-1}[/tex]

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