- #1

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- 2

- Homework Statement
- Determine the rate law for this reaction given the data below.

2 NO + 2 H2 -> N2 + 2H2O

Reaction 1:

Initial [NO] = 0.20

Initial [H2] = 0.15

Initial rate = 2.0 * 10^(-4)

Reaction 2:

Initial [NO] = 0.40

Initial [H2] = 0.15

Initial rate = 8.0 * 10^(-4)

Reaction 3:

Initial [NO] = 0.40

Initial [H2] = 0.30

Initial rate = 1.6 * 10^(-3)

I think the rate law is rate = k[NO][SUP]2[/SUP][H2], since when you double the NO concentration, you quadruple the rate.

The solution is rate = k[NO][H2]. Is this wrong? Thanks.

- Relevant Equations
- rate law

My solution and question are in the homework statement due to some formatting issues. Thanks.