A galvanic cell is assembled at 298 K using a strip of Zn(s) in a 1.0 M solution of ZnCl₂ as the anode compartment and a strip of Cu(s) in a 1.0 M solution of CuSO₄ as the cathode compartment. A salt bridge containing KNO₃ connects the two half-cells. The measured cell potential is 1.03 V, whereas the standard cell potential for the same redox pair is 1.10 V.
For all numerical comparisons, treat the solutions as ideal and assume that activities equal molar concentrations.
(a) Write the balanced overall chemical reaction occurring in the cell under the conditions described.
(b) Express the reaction quotient Q entirely in terms of the aqueous zinc-ion concentration, [Zn²⁺], given that [Cu²⁺] = 1.0 M.
(c) The measured potential (1.03 V) is lower than the standard value (1.10 V). Using this information and your expression for Q, determine whether [Zn²⁺] is greater than, equal to, or less than 1.0 M. Provide a clear chemical justification without performing a full numerical calculation.