Consider the gas-phase reaction between nitric oxide and bromine at 273 °C. 2 NO(g) + Br2(g)→2 NOBr(g) The following data for the initial rate of appearance of NOBr were obtained:
| Experiment |
[NO](M) |
[Br2] (M) |
Initial Rate (M/s) |
| 1 |
0.1 |
0.2 |
24 |
| 2 |
0.25 |
0.2 |
150 |
| 3 |
0.1 |
0.5 |
60 |
| 4 |
0.35 |
0.5 |
735 |
(a) Determine the rate law.
(b) Calculate the average value of the rate constant for the appearance of NOBr from the four data sets.
(c) How is the rate of appearance of NOBr related to the rate of disappearance of Br2?
(d)What is the rate of disappearance of Br2 when [Br2] = 0.25 M and [NO] = 0.075 M ?