(B) The given reactions are oxidation half-reactions:$Zn \to Zn^{2+} + 2e^-; E^o_{ox} = 0.76 \, V$$Fe \to Fe^{2+} + 2e^-; E^o_{ox} = 0.44 \, V$For the

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

(B) The given reactions are oxidation half-reactions:$Zn \to Zn^{2+} + 2e^-; E^o_{ox} = 0.76 \, V$$Fe \to Fe^{2+} + 2e^-; E^o_{ox} = 0.44 \, V$For the cell reaction $Fe^{2+} + Zn \to Zn^{2+} + Fe$,the oxidation occurs at the $Zn$ electrode (anode) and reduction occurs at the $Fe$ electrode (cathode).$E^o_{cell} = E^o_{cathode(red)} - E^o_{anode(red)}$Since $E^o_{red} = -E^o_{ox}$:$E^o_{cathode(red)} = -E^o(Fe \to Fe^{2+}) = -0.44 \, V$$E^o_{anode(red)} = -E^o(Zn \to Zn^{2+}) = -0.76 \, V$$E^o_{cell} = -0.44 - (-0.76) = -0.44 + 0.76 = +0.32 \, V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

The oxidation potentials of the following half-cell reactions are given:
$Zn \to Zn^{2+} + 2e^-; E^o = 0.76 \, V$
$Fe \to Fe^{2+} + 2e^-; E^o = 0.44 \, V$
What will be the $EMF$ of the cell whose cell reaction is:
$Fe^{2+}_{(aq)} + Zn \to Zn^{2+}_{(aq)} + Fe$

A
$-1.20 \, V$
B
$+0.32 \, V$
C
$-0.32 \, V$
D
$+1.20 \, V$

Explore More

Browse All

Question Bank

All Subjects

Class 12 Questions

Class 12

Chemistry Questions

Chapter

Electrochemistry

Subtopic

Electrode potential and ECell

Write the equation relating thermodynamics and electrochemistry.

Easy

View Solution

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 $V$)

MediumWBJEE 2014

View Solution

The standard reduction potentials (in $V$) of a few metal ion/metal electrodes are given below: $Cr^{3+}/Cr = -0.74$; $Cu^{2+}/Cu = +0.34$; $Pb^{2+}/Pb = -0.13$; $Ag^{+}/Ag = +0.8$. The reducing strength of the metals follows the order:

MediumKVPY 2015

View Solution

Standard reduction potentials for the following reactions are :
$Fe^{3+} + 3e^{-} \rightarrow Fe ; E^{\circ}_{1} = -0.036 \ V$
$Fe^{2+} + 2e^{-} \rightarrow Fe ; E^{\circ}_{2} = -0.44 \ V$
What will be the standard electrode potential for
$Fe^{3+} + e^{-} \rightarrow Fe^{2+} (in $V$)?$

Easy

View Solution

For the decomposition of $Al_2O_3$ at $500^{\circ}C$,the free energy change is $\frac{2}{3} Al_2O_3 \to \frac{4}{3} Al + O_2$,$\Delta G = +966 \ kJ \ mol^{-1}$. The potential difference required for the electrolytic reduction of $Al_2O_3$ at $500^{\circ}C$ is ........... $V$.

Medium

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 oxidation potentials of the following half-cell reactions are given:$Zn \to Zn^{2+} + 2e^-; E^o = 0.76 \, V$$Fe \to Fe^{2+} + 2e^-; E^o = 0.44 \, V$What will be the $EMF$ of the cell whose cell reaction is:$Fe^{2+}_{(aq)} + Zn \to Zn^{2+}_{(aq)} + Fe$

Similar Questions

Write the equation relating thermodynamics and electrochemistry.

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 $V$)

The standard reduction potentials (in $V$) of a few metal ion/metal electrodes are given below: $Cr^{3+}/Cr = -0.74$; $Cu^{2+}/Cu = +0.34$; $Pb^{2+}/Pb = -0.13$; $Ag^{+}/Ag = +0.8$. The reducing strength of the metals follows the order:

Standard reduction potentials for the following reactions are : $Fe^{3+} + 3e^{-} \rightarrow Fe ; E^{\circ}_{1} = -0.036 \ V$ $Fe^{2+} + 2e^{-} \rightarrow Fe ; E^{\circ}_{2} = -0.44 \ V$ What will be the standard electrode potential for $Fe^{3+} + e^{-} \rightarrow Fe^{2+} (in $V$)?$

For the decomposition of $Al_2O_3$ at $500^{\circ}C$,the free energy change is $\frac{2}{3} Al_2O_3 \to \frac{4}{3} Al + O_2$,$\Delta G = +966 \ kJ \ mol^{-1}$. The potential difference required for the electrolytic reduction of $Al_2O_3$ at $500^{\circ}C$ is ........... $V$.

Vedclass Test Series

Exam Paper Generator

Online Exam Module

The oxidation potentials of the following half-cell reactions are given:
$Zn \to Zn^{2+} + 2e^-; E^o = 0.76 \, V$
$Fe \to Fe^{2+} + 2e^-; E^o = 0.44 \, V$
What will be the $EMF$ of the cell whose cell reaction is:
$Fe^{2+}_{(aq)} + Zn \to Zn^{2+}_{(aq)} + Fe$

Standard reduction potentials for the following reactions are :
$Fe^{3+} + 3e^{-} \rightarrow Fe ; E^{\circ}_{1} = -0.036 \ V$
$Fe^{2+} + 2e^{-} \rightarrow Fe ; E^{\circ}_{2} = -0.44 \ V$
What will be the standard electrode potential for
$Fe^{3+} + e^{-} \rightarrow Fe^{2+} (in $V$)?$