For the reaction , the rate of disappearance of is . What is the rate of formation of in ? Express y — Chemical Kinetics Chemistry Question
Question
For the reaction $2SO_2 + O_2 \rightarrow 2SO_3$, the rate of disappearance of $SO_2$ is $1.28 \times 10^{-3} \text{ g s}^{-1}$. What is the rate of formation of $SO_3$ in $\text{g s}^{-1}$? Express your answer as $X \times 10^{-3}$ and provide the value of $X$. (Molar mass of $SO_2 = 64 \text{ g mol}^{-1}$, $SO_3 = 80 \text{ g mol}^{-1}$)
Answer: 1.6
💡 Solution & Explanation
Rate in moles: $-\frac{d[SO_2]}{dt} = \frac{1.28 \times 10^{-3}}{64} = 2 \times 10^{-5} \text{ mol s}^{-1}$. Since stoichiometry of $SO_2$ and $SO_3$ is 2:2, $\frac{d[SO_3]}{dt} = 2 \times 10^{-5} \text{ mol s}^{-1}$. Mass rate of $SO_3 = 2 \times 10^{-5} \times 80 = 1.6 \times 10^{-3} \text{ g s}^{-1}$. Thus, $X = 1.6$.
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