Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction rate constant 1 NO₂(g) - NO(g) + O(g) k₁ 2 O(g) + NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₁»k₂. That is, the first step is much faster than the second. Write the balanced 0 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 for Check constants l Explanation rate = k k =
Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction rate constant 1 NO₂(g) - NO(g) + O(g) k₁ 2 O(g) + NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₁»k₂. That is, the first step is much faster than the second. Write the balanced 0 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 for Check constants l Explanation rate = k k =
Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction rate constant 1 NO₂(g) - NO(g) + O(g) k₁ 2 O(g) + NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₁»k₂. That is, the first step is much faster than the second. Write the balanced 0 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 for Check constants l Explanation rate = k k =
Suppose the formation of nitrosyl chloride 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.
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.
Transcribed Image Text:Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism:
step
elementary reaction
rate constant
1
NO₂(g)
→
NO(g) + O(g)
k₁
2 O(g) + NO₂(g) → O₂(g) + NO(g)
k₂
Suppose also k₁»k₂. That is, the first step is much faster than the second.
Write the balanced
0
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
and I
for
Check
constants l
Explanation
rate = k
k =
Transcribed Image Text:Writing the rate law implied by a simple mechanism
NO₂(g) → NO(g) + V(g)
k₁
2 O(g) + NO₂(g) → O₂(g) + NO(g)
k₂
Suppose also k₁k₂. That is, the first step is much faster than the second.
Write the balanced
chemical equation for the
overall chemical reaction:
0
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.
Explanation
Check
rate =
k =
0
k0
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
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