Copper is oxidized by nitric acid. If this property were utilized in an electrochemical cell, what would the standard cell potential be? The relevant reduction reactions and standard reduction potentials are given below. +0.34 V
Cu²⁺ + 2e^- $\rightarrow$ Cu
+0) 96 V
NO₃^- + 4H⁺ + 3e^- $\rightarrow$ NO + 2H₂O

Question

Copper is oxidized by nitric acid. If this property were utilized in an electrochemical cell, what would the standard cell potential be? The relevant reduction reactions and standard reduction potentials are given below. +0.34 V
Cu²⁺ + 2e^-

\rightarrow

Cu
+0) 96 V
NO₃^- + 4H⁺ + 3e^-

\rightarrow

NO + 2H₂O

Quizplus · Accepted Answer

The standard cell potential is calculated by subtracting the standard reduction potential of the anode from the cathode. Here, the cathode is the reduction of NO3^- with a potential of +0.96 V, and the anode is the oxidation of Cu with a potential of -0.34 V (reverse of the given reduction potential). Thus, E°cell = 0.96 V - (-0.34 V) = +0.62 V.

Copper Is Oxidized by Nitric Acid →\rightarrow→ Cu +0)96 V NO3- + 4H+ + 3e-

Copper Is Oxidized by Nitric Acid $\rightarrow$ Cu
+0)96 V
NO₃^- + 4H⁺ + 3e^-