Word Count : 313

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We are given the equilibrium reaction: $$ 2\mathrm{SO}_2(g) + \mathrm{O}_2(g) \rightleftharpoons 2\mathrm{SO}_3(g) \quad \text{with} \quad K_c = 245 \text{ at 100 K} $$ ### Given Equilibrium Concentrations: $$ [\mathrm{SO}_2] = 0.204 \, \text{mol/L}, \quad [\mathrm{O}_2] = 0.0264 \, \text{mol/L}, \quad [\mathrm{SO}_3] = 0.368 \, \text{mol/L} $$ We are asked to determine whether doubling the concentration of SO₂ will shift the reaction toward the reactant side. --- ## Step 1: Write Expression for $K_c$ $$ K_c = \frac{[\mathrm{SO}_3]^2}{[\mathrm{SO}_2]^2 [\mathrm{O}_2]} __________ _______ ________ ________ _________ _______ _________ _________ ___ _________ _____ ____.
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