For the following combination reaction,

2 NO2(g) + F2(g) = 2 NO2F(g)

The initial rates of this reaction were determined for several concentrations of the reactants. All of the data is summarized via the following table:

Experiment [NO2] (M) [F2] (M) Rate (M/s)

1 0.100 0.100 0.026

2 0.200 0.100 0.051

3 0.200 0.200 0.103

4 0.400 0.400 0.411

a) Determine the rate law for this reaction based on the data above.

b) Calculate the rate constant, with appropriate units.

Question

For the following combination reaction,

2 NO2(g) + F2(g) = 2 NO2F(g)

The initial rates of this reaction were determined for several concentrations of the reactants. All of the data is summarized via the following table:

Experiment	[NO2] (M)	[F2] (M)	Rate (M/s)
1	0.100	0.100	0.026
2	0.200	0.100	0.051
3	0.200	0.200	0.103
4	0.400	0.400	0.411

a) Determine the rate law for this reaction based on the data above.

b) Calculate the rate constant, with appropriate units.

	a.	rate = k [NO₂] [F₂]²
	b.	rate = k [NO₂] [F₂]
	c.	rate = k [F₂]²
	d.	rate = k [NO₂]² [F₂]

Experiment	[A]o (M)	[B]o (M)	[C]o (M)	Rate (M*min-1)
1	0.100	0.100	0.100	5.00
2	0.125	0.100	0.200	7.81
3	0.100	0.250	0.300	12.5
4	0.320	0.200	0.400	102.4

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[NO₂], (M)	[F₂] (M)	Initial Rate (M/s)
0.100	0.100	0.026
0.200	0.100	0.025
0.200	0.200	0.103
0.400	0.400	0.411