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December 21, 2014

December 21, 2014

Posted by **Amy** on Wednesday, January 30, 2013 at 12:51am.

2NO2 (g) + F2 (g) ->2NO2F(g)

A: Calculate the value of the rate constant, k.

B: What is the overall order of the reaction?

- Kinetics Problem II -
**DrBob222**, Wednesday, January 30, 2013 at 12:53amNo data.

- Kinetics Problem II -
**Amy**, Wednesday, January 30, 2013 at 11:48amHere is the data. I am sorry that I forgot to list it:

Initial Rate

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

0.100 0.100 0.026

0.200 0.100 0.051

0.200 0.200 0.103

0.400 0.400 0.411

- Kinetics Problem II -
**Devron**, Wednesday, January 30, 2013 at 3:18pmInitial Rate

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

0.100 0.100 0.026

0.200 0.100 0.051

0.200 0.200 0.103

0.400 0.400 0.411

When the concentration of NO2 is doubled from line 1 to line 2, the rate doubles. When the concentration of F2 doubles from line 2 to line 3, the rate doubles, so 2^n=2 and 2^m=2

So, n=1 and m=1

rate=k[NO2][F2]

Taking the data from line 1, solve for k

0.026=k[0.1][0.1]

k=(0.026)/([0.1][0.1])

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