Nitric oxide reacts rapidly with unstable nitrogen trioxide NO 3 to form NO 2 NO

Question

Nitric oxide reacts rapidly with unstable nitrogen trioxide NO3 to form NO2

NO(g) + NO3(g) 2NO2(g)

Determine the rate law for the reaction and calculate the rate constant from the data below

Experiment

[NO]o (M)

[NO3 ] (M)

Initial reaction rate (M/s)

1

1.25x10-3

1.25x10-3

2.45 x 104

2

2.50x10-3

1.25x10-3

4.90 x 104

3

2.50x10-3

2.50x10-3

9.80 x 104

Experiment

[NO]o (M)

[NO3 ] (M)

Initial reaction rate (M/s)

1

1.25x10-3

1.25x10-3

2.45 x 104

2

2.50x10-3

1.25x10-3

4.90 x 104

3

2.50x10-3

2.50x10-3

9.80 x 104

Explanation / Answer

Going from experiment 1 to 2, [NO] gets doubled, [NO3] remains same and rate constant also gets doubled. Hence reaction is first order with respect to [NO].

Going from experiment 2 to 3, [NO3] gets doubled, [NO] remains same and rate constant also gets doubled. Hence reaction is first order with respect to [NO3].

Therefore, rate law is given by:

Rate = k[NO][NO3]

Consider experiment 1:

Rate = k[NO][NO3]

2.45 * 104 = k(1.25 * 10-3)(1.25 * 10-3)

k = 1.568 * 10-2 M-1s-1

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