Question

The standard reduction potentials of Cu2+|Cu and Cu2+|Cu+ are 0.337V and 0.153V, respectively.The standard electrode potential of Cu+|Cu half cell is

Answer 1

Answer:0.521 V

Explanation: it is solve by Δg = -nfE

Answer 2

Given:

Standard reduction potential of $Cu^{2+}|Cu$ = 0.337V

Standard reduction potential of $Cu^{2+}|Cu^+$ = 0.153V

To find:

The standard electrode potential of $Cu^+|Cu$ half cell = ?

Formula to be used:

ΔG° = -nFE°

Calculation:

$Cu^{2+} + 2e^-\rightarrow Cu$  - 1

ΔG° of 1 = $-(2) (F) (0.337 V)$

$Cu^{2+}+ e^-\rightarrow Cu^+$  - 2

ΔG° of 2 = $-(1) (F) (0.153V)$

When eqution 1 and 2 are subtarcted it gives

$Cu^+ + e^-\rightarrow Cu$

ΔG° for the obtained equation is

ΔG° = ΔG° of 1 - ΔG° of 2

ΔG° = -(4)F{(2 × 0.337 - 0.153)}

$E_{Cu^+|Cu} = 2 \times0.337 - 0.153 = 0.521V$

Conclusion:

The standard electrode potential of Cu+|Cu half cell is 0.521V.

Learn more about the standard electrode potential

Question 8.29 Given the standard electrode potentials,

K+/K = –2.93V, Ag+/Ag = 0.80V,

Hg2+/Hg = 0.79V

Mg2+/Mg = –2.37V. Cr3+/Cr = –0.74V

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