Match each equilibrium scenario in Column I with the correct outcome in Column II. Column I (only the given reactants are present initially): (i) NH4I(s) = NH3(g) + HI(g); pressure is increased at equilibrium. (ii) N2(g) + 3H2(g) = 2NH3(g); volume is increased at equilibrium. (iii) H2O(g)

Question

Match each equilibrium scenario in Column I with the correct outcome in Column II. Column I (only the given reactants are present initially): (i) NH4I(s) = NH3(g) + HI(g); pressure is increased at equilibrium. (ii) N2(g) + 3H2(g) = 2NH3(g); volume is increased at equilibrium. (iii) H2O(g) + CO(g) = H2(g) + CO2(g); an inert gas is added at constant total pressure at equilibrium. (iv) PCl5(g) = PCl3(g) + Cl2(g); Cl2 is removed at equilibrium. Column II: (p) Equilibrium shifts forward. (q) No shift in equilibrium. (r) Equilibrium shifts backward. (s) Final pressure exceeds initial pressure.

Accepted Answer

I -> r; II -> r; III -> q; IV -> p. (i) NH4I(s) = NH3(g)+HI(g): both products are gases. Increasing pressure shifts toward fewer gas moles = backward (r). (ii) N2+3H2=2NH3: delta-n = 2-4 = -2. Increasing volume = decreasing pressure shifts toward more moles = left = backward (r). (iii) H2O(g)+CO(g)=H2(g)+CO2(g): delta-n=0. Adding inert gas at constant pressure expands the system but partial pressures of reactants/products are unchanged (volume increases proportionally). No shift (q). (iv) PCl5=PCl3+Cl2: removing Cl2 shifts forward (p). So I-r, II-r, III-q, IV-p.

Solution

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