The following data were collected for the reaction between hydrogen and nitric oxide at 1280c.
2NO (g) + 2H2 (g) ------> 2H2O (g) +N2 (g)
Intial concentrations: Intial Rate:
Expt 1 NO: 5.0 x 10^-3 M H2: 2.0 x 10^-3 M 1.3 x 10^-5 M/s
Expt 2 NO: 10.0 x 10^-3 M H2: 2.0 x 10^-3 M 5.0 x 10^-5 M/s
Expt 3 NO: 10.0 X 10^-3 M H2: 4.0 x 10^-3 M 10.0 x 10^-5 M/s
1. Determine the order of the reaction
2. what is the rate law?
3. what is the value of the rate constant?
The following data were collected for the reaction between hydrogen and nitric oxide at 1280c.
2NO (g) + 2H2 (g) ------> 2H2O (g) +N2 (g)
Intial concentrations: Intial Rate:
Expt 1 NO: 5.0 x 10^-3 M H2: 2.0 x 10^-3 M 1.3 x 10^-5 M/s
Expt 2 NO: 10.0 x 10^-3 M H2: 2.0 x 10^-3 M 5.0 x 10^-5 M/s
Expt 3 NO: 10.0 X 10^-3 M H2: 4.0 x 10^-3 M 10.0 x 10^-5 M/s
1. Determine the order of the reaction
2. what is the rate law?
3. what is the value of the rate constant?
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Related questions
The following data were collected for the reaction between hydrogen and nitric oxide at 700 C:
2H2(g)+2NO(g) -> 2H2O(g)+N2(g)
| Experiment | [H2]/M | [NO]/M | initial rate/M*s-1 |
|---|---|---|---|
| 1 | 0.010 | 0.025 | 2.4x10-6 |
| 2 | 0.0050 | 0.025 | 1.2x10-6 |
| 3 | 0.010 | 0.0125 | 0.60x10-6 |
a) What is the rate law for the reaction?
b) Calculate the rate constant for the reaction
c) More careful studies if the reaction show that the rate law over a wide range of concentrations of reactants should be:
rate= (k1[NO]2[H2])/(1+k2[H2])
What happens to the rate law at very high and very low hydrogen concentrations?
