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Consider the following reaction: 2NO (g) + 2H2 (g) ----> N2 (g) +2H2O (g). The reaction is first-order with respect to H2 and second-order with respect to NO.
A) Write the rate law for this reaction.
B) What is the overall order of this reaction?
C) What happens to the rate if both [NO] and [H2] are tripled?
Consider the following reaction: 2NO (g) + 2H2 (g) ----> N2 (g) +2H2O (g). The reaction is first-order with respect to H2 and second-order with respect to NO.
A) Write the rate law for this reaction.
B) What is the overall order of this reaction?
C) What happens to the rate if both [NO] and [H2] are tripled?
Jarrod RobelLv2
16 Jan 2019
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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?
