Given the following balanced equation,determine the rate of reaction with respect to [O₂].If the rate of O₂ loss is 2.64 × 10^-3 M/s,what is the rate of formation of SO₃? 2 SO₂(g)+ O₂(g)→ 2 SO₃(g)

Question

Quizplus · Accepted Answer

Given the stoichiometry of the reaction, the rate of formation of $\text{SO}_3$ is twice the rate of loss of $\text{O}_2$ because for every 1 mole of $\text{O}_2$ consumed, 2 moles of $\text{SO}_3$ are produced. Therefore, if the rate of $\text{O}_2$ loss is $2.64 \times 10^{-3} \, \text{M/s}$, the rate of $\text{SO}_3$ formation is $2 \times 2.64 \times 10^{-3} = 5.28 \times 10^{-3} \, \text{M/s}$.

Given the Following Balanced Equation,determine the Rate of Reaction with Respect