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Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism: step elementary reaction rate constant (g) (g) (g) (g) (g) (g) Suppose also ≫. That is, the first step is much faster than the second.

Write the balanced chemical equation for the overall chemical reaction:
Write the experimentally-observable rate law for the overall chemical reaction.

Note: your answer should not contain the concentrations of any intermediates.

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Answer:

Koverall [NO]^2 [Br2]

Balanced chemical reaction equation;

2NO + Br2 ⇄2NOBr

Explanation:

Consider the first step in the reaction;

NO(g) + Br2(g) ⇄ NOBr2(g) fast

The second step is the slower rate determining step

NOBr2(g) + NO(g) ⇄ 2NOBr(g)

Given that k1= [NOBr2]/[NO] [Br2]

k2= [NOBr2] [NO]

The concentration of the intermediate is now;

[NOBr2]= k1[NO][Br2]

It then follows that overall rate of reaction is

Rate= k1k2[NO]^2 [Br2]

Since k1k2=Koverall

Rate= Koverall [NO]^2 [Br2]

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