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?

Question

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?

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