Question

What is the overall order of the following reaction, given the rate law? NO(g) + O3(g) â NO2(g) + O2(g) Rate = k[NO][03] A) 1st order B) 2nd order C) 3rd order D) Zero order

Answer 1

The reaction NO(g) + O3(g) â NO2(g) + O2(g) with the rate law Rate = k[NO][O3] is second order overall, as it is first order with respect to NO and first order with respect to O3.

Step-by-step explanation:

The overall order of a reaction is the sum of the exponents of the concentration terms in the rate equation. In the given rate law Rate = k[NO][O3], the reaction is first order with respect to both NO and O3 because the concentrations of NO and O3 are each raised to the first power. Therefore, the overall order of the reaction is the sum of the exponents, which is 1 + 1 = 2. This means the correct answer is B) 2nd order.

Answer 2

The correct option is: B) 2nd order

Step-by-step explanation:

The rate law equation of a chemical reaction is a mathematical expression which expresses the relationship of the rate of the chemical reaction with concentration of reactants. The overall order of the reaction is equal to the sum of orders with respect to all the reactants in the rate law equation.

The given reaction: NO(g) + O₃(g) → NO₂(g) + O₂(g)

Rate = k[NO][O₃]

Therefore, the given chemical reaction is second order.