Question

What can be deduced from the following information?
$2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right);\Delta H=-98kJmo{l}^{-1}$

• A. Increasing the pressure increases the equilibrium yield of $S{O}_3\left(g\right)$
• B. The maximum mass of sulphur trioxide that can be made from $64$ g sulphur dioxide is $90$ g
• C. Increasing the temperature increases the rate of the forward reaction
• D. Increasing the pressure increase the equilibrium yield of $S{O}_2$

Answer 1

Answer: (A)

Increasing the pressure increases the equilibrium yield of $S{O}_3\left(g\right)$

For an equilibrium reaction, the increment in pressure will lead to the reaction in a direction where moles decreases.

So increasing the pressure will lead the reaction in a forward direction and increase the yield of the $S{O}_3$

The given reaction is an exothermic reaction. With an increase in temperature, the reaction will compensate it by absorbing the excess heat produced. For this, the reaction will move towards the endothermic side. Thus, the backward reaction will be favoured.