Question

1 Hydrogen gas reduces NO to N2 in the following reaction:

2H2 (g) +2 NO (g) ⇌ 2H2O (g) + N2(g)

The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results:

Experiment [H2]0 (M) [NO]0 (M) Initial Rate (M/s)

1 0.212 0.136 0.0221

2 0.212 0.272 0.0445

3 0.424 0.544 0.349

4 0.848 0.544 1.40

a) what is the rate la for the reaction at 1500°C?

b) Determine the rate constant for the reaction at 1500°C?

Answer 1

$rate = k [NO]^2 [H2]$

From experiment 1 and 2

$rate=dC/dT$ =0.136/1500= 9.07*10^-5

9.07*10^-5= K(0.272)²(0.212)

K=5.78M^-2S^-1