Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (aughing gas) according to the equation: H2 (g) + 2NO(g) → N2O(g) + H2O(g)Based on the following data: Trail 1 Trail 2 Trail 3H2 (M) 0.30 0.60 0.60NO (M) 0.35 0.35 0.70Rate (M*s) 2.835 x 10^-3 1.134 x 10^-2 2.268 x 10^-2Required:a. What is the order with respect to H2? b. What is the order with respect to NO? c. What is the rate equation for this reaction? d. Calculate the rate constant for the reaction.

Explanation:

H2 (g) + 2NO(g) → N2O(g) + H2O(g)

Trial 1 Trial 2 Trial 3

H2 (M) 0.30 0.60 0.60

NO (M) 0.35 0.35 0.70

Rate (M*s) 2.835 x 10^-3 1.134 x 10^-2 2.268 x 10^-2

a. What is the order with respect to H2?

Comparing trial 1 and 2, the conc of H2 is doubled, the rate of the reaction increased by a factor f 4. This means the rate is in second order with respect to H2.

b. What is the order with respect to NO?

Comparing Trial 2 and 3, the concentration of NO is doubled, the rate of the reaction increased by a factor of 2. This means the rate is in first order with respect to NO.

c. What is the rate equation for this reaction?

The rate equation is given as;

rate = k [H2]²[NO]

d. Calculate the rate constant for the reaction.

Taking trial 1;

2.835 x 10^-3 = k (0.30)²(0.35)

k = 2.835 x 10^-3  / 0.0315 = 90  x 10^-3

k = 0.09 L2 mol-2 s-1