Question

Consider the reaction between nitrogen dioxide and carbon monoxide:

NO2(g) + CO(g) + NO(g) + CO2(g)

Experiment [NO2] (M) [CO] (M) Initial Rate (M)
1 0.182 0.182 0.3636
2 0.364 0.182 1.4545
3 0.364 0.364 1.4545

k = ?

Answer 1

The rate law for the reaction between NO2 and CO at 100 °C is second order in NO2 and zero order in CO, leading to the rate equation rate = k[NO2]², where k is the rate constant.

Step-by-step explanation:

The question pertains to determining the rate law and the rate constant (k) for a chemical reaction involving nitrogen dioxide (NO2) and carbon monoxide (CO) at 100 °C.

Based on the provided data and the fact that the reaction is second order in NO2 and zero order in CO, we can write the rate law as rate = k[NO2]². As CO is zero order, its concentration does not affect the rate of reaction and can therefore be omitted from the rate law equation.

Using the given initial rates and concentrations from the experiments, we can solve for the rate constant (k), which can be determined from any of the experiments since for a given temperature, the rate constant should be the same.