Question

The following reaction goes to completion:

2NO(g) + H2(g) ⇌ N2O(g) + H2O(g) + 340,270J
What would be the effect on the reaction rate if the hydrogen gas concentration were doubled?
If the pressure on the reaction were doubled?

Answer 1

The effect on the reaction rate if the hydrogen gas concentration were doubled would depend on the rate law of the reaction. If the rate law is rate = k[NO]²[H₂], doubling the concentration of H₂ would quadruple the rate of the reaction. If the rate law is rate = k[NO]²[H₂]², doubling the concentration of H₂ would increase the rate by a factor of 16.

Step-by-step explanation:

The effect on the reaction rate if the hydrogen gas concentration were doubled would depend on the rate law of the reaction. The rate law can be determined experimentally and represents the relationship between the concentration of the reactants and the rate of the reaction.

If the rate law is given as rate = k[NO]²[H₂], then doubling the concentration of H₂ would result in a rate that is 2² = 4 times greater. This means that doubling the concentration of H₂ would quadruple the rate of the reaction.

On the other hand, if the rate law is given as rate = k[NO]²[H₂]², then doubling the concentration of H₂ would result in a rate that is 2²² = 16 times greater. This means that doubling the concentration of H₂ would increase the rate of the reaction by a factor of 16.