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 |
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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