⇒Thermodynamics

Correct Option is (A)

For oxidation of 4 moles of ${\mathrm{SO}}_2$, the reaction is given as follows:

$4{\mathrm{SO}}_{2(\mathrm{g})}+2{\mathrm{O}}_{2(\mathrm{g})}⟶4{\mathrm{SO}}_{3(\mathrm{g})}$

$\mathrm{\Delta }{\mathrm{n}}_{\mathrm{g}}=$ (moles of product gases) $-$ (moles of reactant gases)

$\begin{array}{rl}\mathrm{\Delta }{\mathrm{n}}_{\mathrm{g}}& =4-6=-2\mathrm{mol}\\ \mathrm{W}& =-\mathrm{\Delta }{\mathrm{n}}_{\mathrm{g}}\mathrm{RT}\\ & =-(-2\mathrm{mol})\times 8.314\mathrm{J}{\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}\times 300\mathrm{K}\\ & =+4988.4\mathrm{J}\\ & =+4.988\mathrm{kJ}\end{array}$

[Note: For the given question, none of the provided options is the correct answer.]