A scientist conducts an experiment to determine the rate of NO formation in the following reaction: 2 N₂O₅(g) $\rightarrow$ 4 NO₂(g) + O₂(g)
If the initial concentration of N₂O₅ was 0.500 M and the concentration of N₂O₅ was 0.450 M after 0.100 s, what is the average rate of NO₂ formation during the first 100 milliseconds?

Question

A scientist conducts an experiment to determine the rate of NO formation in the following reaction: 2 N₂O₅(g)

\rightarrow

4 NO₂(g) + O₂(g)
If the initial concentration of N₂O₅ was 0.500 M and the concentration of N₂O₅ was 0.450 M after 0.100 s, what is the average rate of NO₂ formation during the first 100 milliseconds?

Quizplus · Accepted Answer

The average rate of $NO_2$ formation is calculated based on the change in concentration of $N_2O_5$ over time, considering the stoichiometry of the reaction. The initial concentration of $N_2O_5$ is 0.500 M, and after 0.100 s, it is 0.450 M. This means $N_2O_5$ has decreased by 0.050 M in 0.100 s. The reaction shows that 2 moles of $N_2O_5$ produce 4 moles of $NO_2$, so the rate of $NO_2$ formation is twice the rate of $N_2O_5$ depletion. Therefore, the rate of $NO_2$ formation is $(0.050 M / 0.100 s) \times 2 = 1.0 M/s$.

A Scientist Conducts an Experiment to Determine the Rate of NO