Consider the following reaction:
2Cu⁺(aq) $\rightarrow$ Cu(s) + Cu²⁺(aq) If the standard potentials of Cu²⁺ and Cu⁺ are +0.34 and +0.52 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

Question

Consider the following reaction:
2Cu⁺(aq)

\rightarrow

Cu(s) + Cu²⁺(aq) If the standard potentials of Cu²⁺ and Cu⁺ are +0.34 and +0.52 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

Quizplus · Accepted Answer

The standard cell potential ($E^\circ_{cell}$) for the reaction is calculated using the formula: $E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode}$. Given that the standard potentials for Cu^2+ + 2e^- → Cu(s) is +0.34 V and for Cu^+ + e^- → Cu(s) is +0.52 V, the reaction as written shows Cu^+ being oxidized to Cu^2+ and Cu being reduced from Cu^2+, making Cu^2+ the cathode and Cu^+ the anode. Therefore, $E^\circ_{cell} = 0.34 V - 0.52 V = -0.18 V$. However, the sign must be considered in the context of the reaction direction, and the correct interpretation leads to a positive value for the cell potential in the context of the given reaction, indicating a mistake in the sign interpretation. The correct calculation without considering sign inversion mistakenly suggests $E^\circ_{cell} = 0.18 V$, but the correct approach to calculate $E^\circ_{cell}$ should consider the actual roles of cathode and anode in the electrochemical series, leading to a reevaluation of the answer.

Consider the Following Reaction: 2Cu+(aq) →\rightarrow→ Cu(s)+ Cu2+(aq)If the Standard Potentials of Cu2+ and Cu+ Are

Consider the Following Reaction:
2Cu⁺(aq) $\rightarrow$ Cu(s)+ Cu²⁺(aq)If the Standard Potentials of Cu²⁺ and Cu⁺ Are