Math / Word Problems

QuestionWhat happens to the equilibrium when $\mathrm{SO}_{3}$ gas is removed from this reaction?
$2 \mathrm{SO}_{2} + \mathrm{O}_{2} \rightleftharpoons 2 \mathrm{SO}_{3} + 198 \mathrm{~kJ}$
A. Shift right, decrease $\mathrm{SO}_{2}$ and $\mathrm{O}_{2}$ .
B. Shift left, increase $\mathrm{O}_{2}$ .
C. Shift left, increase $\mathrm{SO}_{2}$ .
D. No change, remains at equilibrium.

Studdy Solution
When the reaction shifts to the right, it uses up the reactants $\mathrm{}_{2}$ and $\mathrm{}_{2}$ . This means that the concentrations of $\mathrm{}_{2}$ and $\mathrm{}_{2}$ will decrease.
Therefore, the correct answer is A. The reaction will shift toward the products (right) and decrease the concentrations of $\mathrm{}_{2}$ and $\mathrm{}_{2}$ .

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