For the standard cell, Cu(s) | Cu²+(aq) || Ag⁺ (aq) | Ag(s)
Given: E° _Cu²⁺/Cu = 0.34V, E° = 0.80V
(a) Identify cathode and anode as the current is drawn through the cell.
(b) Write the reactions taking place at the electrodes.
(c) Calculate the standard cell potential.

Solution

$a) E_{\frac{{Cu}^{2 +}}{Cu}}^{0} < E_{\frac{{Ag}^{+}}{Ag}}^{0} Therefore copper electorode isthe anode and silver electrode act as a cathode . The half reaction are : anode : Cu (s) \to {Cu}^{2 +} + 2 e^{-} Cathode : 2 {Ag}^{+} + 2 e^{-} \to 2 Ag b) net reaction : Cu (s) + 2 {Ag}^{+} (aq) \to {Cu}^{2 +} (aq) + 2 Ag (s) c) The potential of the cell is given by E = E_{cell}^{0} - \frac{0.059}{n} \log \frac{[{Cu}^{2 +}]}{[{Ag}^{+}]^{2}} 0 = (+ 0.80 - 0.34) - \frac{0.059}{2} \log \frac{0.01}{[{Ag}^{+}]^{2}} \log [\frac{0.01}{({Ag}^{+})^{2 +}}] = \frac{2 x 0.46}{0.059} = 15.593 taking antilog \frac{0.01}{[{Ag}^{+}]^{2}} = antilog 15.593 = 3.919 x 10^{15} [{Ag}^{+}]^{2} = \frac{0.01}{3.919 x 10^{15}} = 2.55 x 10^{- 18} [{Ag}^{+}] = 1.59 x 10^{- 9} M$

Some More Questions From Electrochemistry Chapter

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

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Electrochemistry

For the standard cell, Cu(s) | Cu²+(aq) || Ag⁺ (aq) | Ag(s)
Given: E° _Cu²⁺/Cu = 0.34V, E° = 0.80V
(a) Identify cathode and anode as the current is drawn through the cell.
(b) Write the reactions taking place at the electrodes.
(c) Calculate the standard cell potential.

Some More Questions From Electrochemistry Chapter

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

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Electrochemistry

For the standard cell, Cu(s) | Cu2+(aq) || Ag+ (aq) | Ag(s)Given: E° Cu2+/Cu = 0.34V, E° = 0.80V(a) Identify cathode and anode as the current is drawn through the cell.(b) Write the reactions taking place at the electrodes.(c) Calculate the standard cell potential.

Some More Questions From Electrochemistry Chapter

The molar conductivity of 0.025 mol L–1 methanoic acid is 46.1 S cm2 mol–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H+) = 349.6 S cm2 mol–1 and λ° (HCOO– ) = 54.6 s cm2 mol–1.

If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

Suggest a list of metals that are extracted electrolytically.

Consider the reaction: Cr2O72– + 14H+ + 6e- → 2Cr3+ + 8H2OWhat is the quantity of electricity in coulombs needed to reduce 1 mol of Cr2O72-?

Write the chemistry of recharging the lead storage battery, highlighting all the materials that are involved during recharging.

Suggest two materials other than hydrogen that can be used as fuels in fuel cells.

Name the electrolyte used in fuel cell?

Can we use copper vessel to store AgNO3 solution ?

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation

For the standard cell, Cu(s) | Cu²+(aq) || Ag⁺ (aq) | Ag(s)
Given: E° _Cu²⁺/Cu = 0.34V, E° = 0.80V
(a) Identify cathode and anode as the current is drawn through the cell.
(b) Write the reactions taking place at the electrodes.
(c) Calculate the standard cell potential.

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

Consider the reaction: Cr₂O₇^2– + 14H⁺ + 6e- → 2Cr³⁺ + 8H₂O
What is the quantity of electricity in coulombs needed to reduce 1 mol of Cr₂O₇^2-?

Can we use copper vessel to store AgNO₃solution ?