Question

The reaction $2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right),\Delta H=-X$ kJ, is favoured by high pressure and high temperature.

• A. True
• B. False

Answer 1

The correct option is B False

For the reaction $2S{O}_2+O_2\iff 2S{O}_3$, $\Delta n=2-(2+1)=-1$
Here, $\Delta n$ is the difference in the total number of gaseous products and total number of gaseous reactants.
The number of moles decreases in the forward reaction from 3 to 2 . Also the number of moles increases in the reverse reaction from 2 to 3.
When the pressure is increased by decreasing the volume at constant temperature, the forward reaction will be favored as the forward reaction occurs with decrease in the number of moles.
The negative value of the enthalpy of the reaction indicates that it is an exothermic reaction. When temperature is lowered, the reaction will proceed in the forward direction so as to liberate heat and nullify the effect of lowering temperature. This will increase the value of the equilibrium constant $K_c$.