1.The equilibrium constant for the disproportionation reaction2Cu+(aq)⟶Cu(s)+Cu2+(aq)2\text{Cu}^+ (aq) \longrightarrow \text{Cu}(s) + \text{Cu}^{2+} (aq)2Cu+(aq)⟶Cu(s)+Cu2+(aq)at 25∘^\circ∘C(ECu+/Cu∘=0.52E^\circ_{\text{Cu}^+/\text{Cu}} = 0.52ECu+/Cu∘=0.52 V, ECu2+/Cu∘=0.16E^\circ_{\text{Cu}^{2+}/\text{Cu}} = 0.16ECu2+/Cu∘=0.16 V) is:a.6×1046 \times 10^46×104b.6×1066 \times 10^66×106c.1.2×1061.2 \times 10^61.2×106d.1.2×10−61.2 \times 10^{-6}1.2×10−6Login to continueOnly logged in users canattempt or see the solution.
