Question

For the gas phase reaction,
$2S{O}_2+O_2\rightleftharpoons 2S{O}_3$; $\Delta H=-x$
carried out in a vessel, the equilibrium concentration of $S{O}_2$ can be increased by :

• A. increasing the temperature.
• B. decreasing the pressure.
• C. removing some oxygen.
• D. none of the above.

Answer 1

Answer: (A), (B), (C)

The correct options are
A increasing the temperature.
B decreasing the pressure.
C removing some oxygen.

The equilibrium concentration of $S{O}_2$ can be increased by increasing the temperature.It shows a exothermic reaction .In exothermic reactions, ($\Delta H<0$) heat is released with the products. When separated molecules join together, enough energy is released to overcompensate for the energy required to break reactant bonds.Thus more of $S{O}_3$ can be formed easily and reaction favours forward direction.

The equilibrium concentration of $S{O}_2$ can be increased by decreasing the pressure.It means the volume is increased, the reaction will shift towards the side of the reaction that has more gaseous particles. Thus towards the backward direction.

The equilibrium concentration of $S{O}_2$ can be increased by removing some oxygen. If reactants are removed, the system will shift to form more reactants.It will favours backward reaction.

Option (A),(B),(C) are correct.