Question:medium

For the reaction: 2SO2 + O2 → 2SO3,
the rate of disappearance of O2 is \( 2 \times 10^{-4} \, \text{mol L}^{-1} \text{s}^{-1} \).
What is the rate of appearance of SO3?

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In rate calculations, use the balanced chemical equation to determine the relationship between reactant disappearance and product formation.
Updated On: Jan 13, 2026
  • \( 2 \times 10^{-4} \) mol L$^{-1}$ s$^{-1}$
  • \( 4 \times 10^{-4} \) mol L$^{-1}$ s$^{-1}$
  • \( 1 \times 10^{-1} \) mol L$^{-1}$ s$^{-1}$
  • \( 6 \times 10^{-4} \) mol L$^{-1}$ s$^{-1}$
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The Correct Option is B

Solution and Explanation

To address the issue, we must ascertain the SO3 formation rate, given the O2 consumption rate for the reaction: 2SO2 + O2 ⇌ 2SO3.

The reaction's stoichiometry dictates the rate correlations: 1 mol O2 yields 2 mol SO3.

Given:

  • Rate of O2 disappearance = \(2 \times 10^{-4}\) mol L-1 s-1
  • The rate of SO3 appearance is double the rate of O2 disappearance, due to the 1:2 stoichiometric ratio between O2 and SO3.

Consequently, the rate of SO3 appearance = 2 × Rate of O2 disappearance = 2 × \(2 \times 10^{-4}\) = \(4 \times 10^{-4}\) mol L-1 s-1.

The confirmed solution is:
\(4 \times 10^{-4}\) mol L-1 s-1.

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