Suppose the decomposition of dinitrogen monoxide proceeds by the following mechanism: elementary reaction N₂O(g) N₂(g) + O(g) k₁ 2 N₂O(g) + O(g) N₂(g) + O₂(g) k₂ Suppose also k₁«k₂. That is, the first step is much slower than the second. step - 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. Express the rate constant k for the overall chemical reaction in terms of K₁, K₂, and (if necessary) the rate constants k.₁ and K-2 for the rouoren of the two 0 rate = k k = 0 rate constant

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Suppose the decomposition of dinitrogen monoxide proceeds by the following mechanism:
elementary reaction
N₂O(g) N₂(g) + O(g)
k₁
2 N₂O(g) + O(g) → N₂(g) + O₂(g)
k₂
Suppose also k₁<<k₂. That is, the first step is much slower than the second.
step
1
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.
Express the rate constant
k for the overall chemical
reaction in terms of k₁, K₂,
and (if necessary) the rate
constants k_₁ and k-2 for
the rovorce of the two
0
rate = k
k
- 0
=
rate constant
Transcribed Image Text:Suppose the decomposition of dinitrogen monoxide proceeds by the following mechanism: elementary reaction N₂O(g) N₂(g) + O(g) k₁ 2 N₂O(g) + O(g) → N₂(g) + O₂(g) k₂ Suppose also k₁<<k₂. That is, the first step is much slower than the second. step 1 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. Express the rate constant k for the overall chemical reaction in terms of k₁, K₂, and (if necessary) the rate constants k_₁ and k-2 for the rovorce of the two 0 rate = k k - 0 = rate constant
Suppose also k₁<<k₂. That is, the first step is much slower 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.
Express the rate constant
k for the overall chemical
reaction in terms of k₁, K₂,
and (if necessary) the rate
constants k_₁ and K-2 for
the reverse of the two
elementary reactions in
the mechanism.
1
0
rate = k
k = 0
Transcribed Image Text:Suppose also k₁<<k₂. That is, the first step is much slower 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. Express the rate constant k for the overall chemical reaction in terms of k₁, K₂, and (if necessary) the rate constants k_₁ and K-2 for the reverse of the two elementary reactions in the mechanism. 1 0 rate = k k = 0
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