Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO, (g)+F2 (g) NO,F (g) + F (g) k1 2 F (g) + NO, (g) –→ NO,F (g) k2 Suppose also k, « k,. 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. rate = k U

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Suppose the formation of nitryl fluoride proceeds by the following mechanism:
step
elementary reaction
rate constant
1 NO, g) +F, (g)
NO,F (g) +F (g)
k1
2
F (g) + NO, (g) → NO,F (g)
k2
Suppose also k, « k,. 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.
rate = k U
Note: your answer should not
contain the concentrations of
any intermediates.
Transcribed Image Text:Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO, g) +F, (g) NO,F (g) +F (g) k1 2 F (g) + NO, (g) → NO,F (g) k2 Suppose also k, « k,. 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. rate = k U Note: your answer should not contain the concentrations of any intermediates.
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