The reaction of nitrogen dioxide with fluorine 2NO2+ F2 → 2NO₂ F - is first order in NO2 and first order in F2. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n (don't enter 1) and concentrations taken to the zero power do not appear. Rate = S In an experiment to determine the rate law, the rate constant was determined to be 1.31 x 10-4 M¹s¹. Using this value for the rate constant, the rate of the reaction when [NO₂] = 4.92 M and [F2] = 4.59 M would be M/s.

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The reaction of nitrogen dioxide with fluorine
2NO2+ F2 → 2NO₂F
is first order in
NO₂ and first order in
F2.
Complete the rate law for this reaction in the box below.
Use the form
k[A] [B]", where '1' is understood for
m,
n ... (don't enter 1) and concentrations taken to the zero power
do not appear.
Rate: =
S
In an experiment to determine the rate law, the rate constant
was determined to be 1.31 × 10-4 M¹s¹. Using this value for
the rate constant, the rate of the reaction when [NO₂] = 4.92 M
and [F2] 4.59 M would be
M/s.
=
Transcribed Image Text:The reaction of nitrogen dioxide with fluorine 2NO2+ F2 → 2NO₂F is first order in NO₂ and first order in F2. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate: = S In an experiment to determine the rate law, the rate constant was determined to be 1.31 × 10-4 M¹s¹. Using this value for the rate constant, the rate of the reaction when [NO₂] = 4.92 M and [F2] 4.59 M would be M/s. =
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