(A) The standard $EMF$ of the cell is calculated as: $E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode}$.Given reduction potentials are $E^{\

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

(A) The standard $EMF$ of the cell is calculated as: $E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode}$.Given reduction potentials are $E^{\circ}_{Ag^{+}/Ag} = 0.7995 \ V$ and $E^{\circ}_{Fe^{3+}/Fe^{2+}} = 0.7710 \ V$.Since $E^{\circ}_{Ag^{+}/Ag} > E^{\circ}_{Fe^{3+}/Fe^{2+}}$, the silver electrode acts as the cathode and the iron electrode acts as the anode.$E^{\circ}_{cell} = 0.7995 \ V - 0.7710 \ V = 0.0285 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

The two half-cell reactions of an electrochemical cell are given as: $Ag^{+} + e^{-} \rightarrow Ag$; $E^{\circ}_{Ag^{+}/Ag} = 0.7995 \ V$ and $Fe^{2+} \rightarrow Fe^{3+} + e^{-}$; $E^{\circ}_{Fe^{3+}/Fe^{2+}} = 0.7710 \ V$. The value of cell $EMF$ will be: (in $V$)

WBJEE 2014 All WBJEE

A
$0.0285$
B
$1.5705$
C
$-0.0285$
D
$-1.5705$

Explore More

Browse All

Question Bank

All Subjects

Class 12 Questions

Class 12

Chemistry Questions

Chapter

Electrochemistry

Subtopic

Electrode potential and ECell

Previous Year

WBJEE 2014 Paper All WBJEE years →

The standard electrode potential for the half-cell reactions are
$Zn^{2+} + 2e^{-} \longrightarrow Zn ; E^{\circ} = -0.76 \ V$
$Fe^{2+} + 2e^{-} \longrightarrow Fe ; E^{\circ} = -0.44 \ V$
The $emf$ of the cell reaction,
$Fe^{2+} + Zn \longrightarrow Zn^{2+} + Fe$ is

EasyKCET 2009

View Solution

The standard potential of a $Co^{2+}|Co$ electrode is $-0.28 \ V$ and the standard potential of the cell $Pt|Ti^{2+}_{(aq)}, Ti^{3+}_{(aq)}||Co^{2+}_{(aq)}|Co_{(s)}$ is $0.09 \ V$. What is the standard oxidation potential of the $Ti^{2+}_{(aq)}|Ti^{3+}_{(aq)}$ electrode? ............. $V$

Medium

View Solution

The standard reduction potential for $Li^{+}/Li$,$Zn^{2+}/Zn$,$H^{+}/H_2$ and $Ag^{+}/Ag$ is $-3.05$,$-0.762$,$0.00$ and $+0.80 \ V$. Which of the following has the highest reducing capacity?

Medium

View Solution

The standard reduction potentials for $Zn^{2+}/Zn$,$Ni^{2+}/Ni$,and $Fe^{2+}/Fe$ are $-0.76 \, V$,$-0.23 \, V$,and $-0.44 \, V$ respectively. For which of the following combinations will the reaction $X + Y^{2+} \rightarrow X^{2+} + Y$ be spontaneous?

Easy

View Solution

For the following cell reaction,$Ag | Ag^{+} | AgCl | Cl^{-} | Cl_2, Pt$
$\Delta G_f^{\circ}(AgCl) = -109 \ kJ/mol$
$\Delta G_f^{\circ}(Cl^{-}) = -129 \ kJ/mol$
$\Delta G_f^{\circ}(Ag^{+}) = 78 \ kJ/mol$
$E^{\circ}$ of the cell is

DifficultAP EAMCET 2009

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

The two half-cell reactions of an electrochemical cell are given as: $Ag^{+} + e^{-} \rightarrow Ag$; $E^{\circ}_{Ag^{+}/Ag} = 0.7995 \ V$ and $Fe^{2+} \rightarrow Fe^{3+} + e^{-}$; $E^{\circ}_{Fe^{3+}/Fe^{2+}} = 0.7710 \ V$. The value of cell $EMF$ will be: (in $V$)

Similar Questions

The standard electrode potential for the half-cell reactions are$Zn^{2+} + 2e^{-} \longrightarrow Zn ; E^{\circ} = -0.76 \ V$$Fe^{2+} + 2e^{-} \longrightarrow Fe ; E^{\circ} = -0.44 \ V$The $emf$ of the cell reaction,$Fe^{2+} + Zn \longrightarrow Zn^{2+} + Fe$ is

The standard potential of a $Co^{2+}|Co$ electrode is $-0.28 \ V$ and the standard potential of the cell $Pt|Ti^{2+}_{(aq)}, Ti^{3+}_{(aq)}||Co^{2+}_{(aq)}|Co_{(s)}$ is $0.09 \ V$. What is the standard oxidation potential of the $Ti^{2+}_{(aq)}|Ti^{3+}_{(aq)}$ electrode? ............. $V$

The standard reduction potential for $Li^{+}/Li$,$Zn^{2+}/Zn$,$H^{+}/H_2$ and $Ag^{+}/Ag$ is $-3.05$,$-0.762$,$0.00$ and $+0.80 \ V$. Which of the following has the highest reducing capacity?

The standard reduction potentials for $Zn^{2+}/Zn$,$Ni^{2+}/Ni$,and $Fe^{2+}/Fe$ are $-0.76 \, V$,$-0.23 \, V$,and $-0.44 \, V$ respectively. For which of the following combinations will the reaction $X + Y^{2+} \rightarrow X^{2+} + Y$ be spontaneous?

For the following cell reaction,$Ag | Ag^{+} | AgCl | Cl^{-} | Cl_2, Pt$ $\Delta G_f^{\circ}(AgCl) = -109 \ kJ/mol$ $\Delta G_f^{\circ}(Cl^{-}) = -129 \ kJ/mol$ $\Delta G_f^{\circ}(Ag^{+}) = 78 \ kJ/mol$ $E^{\circ}$ of the cell is

Vedclass Test Series

Exam Paper Generator

Online Exam Module

The standard electrode potential for the half-cell reactions are
$Zn^{2+} + 2e^{-} \longrightarrow Zn ; E^{\circ} = -0.76 \ V$
$Fe^{2+} + 2e^{-} \longrightarrow Fe ; E^{\circ} = -0.44 \ V$
The $emf$ of the cell reaction,
$Fe^{2+} + Zn \longrightarrow Zn^{2+} + Fe$ is

For the following cell reaction,$Ag | Ag^{+} | AgCl | Cl^{-} | Cl_2, Pt$
$\Delta G_f^{\circ}(AgCl) = -109 \ kJ/mol$
$\Delta G_f^{\circ}(Cl^{-}) = -129 \ kJ/mol$
$\Delta G_f^{\circ}(Ag^{+}) = 78 \ kJ/mol$
$E^{\circ}$ of the cell is