Consider the following reaction. 3 O₂ (g)→2 O₃ (g) At a given instant, the rate of disappearance of [O₂] is 2.35×10^{- 5} M/sec. What is the rate of appearance of [O₃] for this reaction at this moment?

Question

Quizplus · Accepted Answer

The rate of appearance of $[OS_2B_3]$ is calculated by multiplying the rate of disappearance of $[OS_2B_2]$ by the stoichiometric ratio of $[OS_2B_3]$ to $[OS_2B_2]$, which is $2/3$. Therefore, $2.35 \times 10^{-5} \times \frac{2}{3} = 1.57 \times 10^{-5}$ M/sec.

Consider the Following Reaction