(B) The reduction half-reaction is: $Fe^{3+} + e^{-} \rightarrow Fe^{2+}$Using the Nernst equation:$E_{Fe^{3+} \mid Fe^{2+}} = E^0_{Fe^{3+} \mid Fe^{2

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(B) The reduction half-reaction is: $Fe^{3+} + e^{-} \rightarrow Fe^{2+}$Using the Nernst equation:$E_{Fe^{3+} \mid Fe^{2+}} = E^0_{Fe^{3+} \mid Fe^{2+}} - \frac{2.303 \ RT}{nF} \log \frac{[Fe^{2+}]}{[Fe^{3+}]}$Here,$n = 1$,$[Fe^{2+}] = 2.0 \ M$,$[Fe^{3+}] = 0.02 \ M$,$\frac{2.303 \ RT}{F} = 0.059 \ V$,and $E^0 = 0.771 \ V$.Substituting the values:$E = 0.771 - 0.059 \log \left(\frac{2.0}{0.02}\right)$$E = 0.771 - 0.059 \log(100)$$E = 0.771 - 0.059 \times 2$$E = 0.771 - 0.118 = 0.653 \ V$

Class 12 Chemistry Electrochemistry Nernst equation and ECS

Medium

The reduction potential of a half cell consisting of a $Pt$ electrode immersed in $2.0 \ M \ Fe^{2+}$ and $0.02 \ M \ Fe^{3+}$ solution (in $V$) is. Given: $\left(\frac{2.303 \ RT}{F} = 0.059, E^0_{Fe^{3+} \mid Fe^{2+}} = 0.771 \ V\right)$

TS EAMCET 2023 All TS EAMCET

A
$0.543$
B
$0.653$
C
$0.733$
D
$0.822$

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What is the reduction electrode potential (in volts) of a copper electrode when $[Cu^{2+}]=0.01 \ M$ is in a solution at $25^{\circ} C$? $(E^{\circ}$ of $Cu^{2+}/Cu$ electrode is $+0.34 \ V)$

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The cell potential for the following reaction is $0.03305 \ V$ at $298 \ K$. Find the value of $x$ for the reaction: $Zn | Zn^{2+} (0.1 \ M) || Cd^{2+} (x \ M) | Cd$. (Given: $E^{\circ}_{Zn^{2+}/Zn} = -0.76 \ V$,$E^{\circ}_{Cd^{2+}/Cd} = -0.40 \ V$) (in $M$)

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Which of the following is the correct expression for the electrode potential of a cell?

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Calculate the cell potential for the following cell: ............... $V$
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Given: $E^0_{Cr^{3+}|Cr} = -0.72 \, V$,$E^0_{Fe^{2+}|Fe} = -0.42 \, V$ (in $, V$)

Easy

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Which of the following is correct as a Nernst equation for the given electrochemical cell ?
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The reduction potential of a half cell consisting of a $Pt$ electrode immersed in $2.0 \ M \ Fe^{2+}$ and $0.02 \ M \ Fe^{3+}$ solution (in $V$) is. Given: $\left(\frac{2.303 \ RT}{F} = 0.059, E^0_{Fe^{3+} \mid Fe^{2+}} = 0.771 \ V\right)$

Similar Questions

What is the reduction electrode potential (in volts) of a copper electrode when $[Cu^{2+}]=0.01 \ M$ is in a solution at $25^{\circ} C$? $(E^{\circ}$ of $Cu^{2+}/Cu$ electrode is $+0.34 \ V)$

The cell potential for the following reaction is $0.03305 \ V$ at $298 \ K$. Find the value of $x$ for the reaction: $Zn | Zn^{2+} (0.1 \ M) || Cd^{2+} (x \ M) | Cd$. (Given: $E^{\circ}_{Zn^{2+}/Zn} = -0.76 \ V$,$E^{\circ}_{Cd^{2+}/Cd} = -0.40 \ V$) (in $M$)

Which of the following is the correct expression for the electrode potential of a cell?

Calculate the cell potential for the following cell: ............... $V$$Cr_{(s)} | Cr^{3+}_{(0.1 \, M)} || Fe^{2+}_{(0.01 \, M)} | Fe_{(s)}$Given: $E^0_{Cr^{3+}|Cr} = -0.72 \, V$,$E^0_{Fe^{2+}|Fe} = -0.42 \, V$ (in $, V$)

Which of the following is correct as a Nernst equation for the given electrochemical cell ?$Mg_{(s)}|Mg_{(aq)}^{2+}(0.1 \ M)||Cl_{(aq)}^{-}(0.1 \ M)|Cl_{2_{(g)}}(1 \ bar)|Pt_{(s)}$

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Calculate the cell potential for the following cell: ............... $V$
$Cr_{(s)} | Cr^{3+}_{(0.1 \, M)} || Fe^{2+}_{(0.01 \, M)} | Fe_{(s)}$
Given: $E^0_{Cr^{3+}|Cr} = -0.72 \, V$,$E^0_{Fe^{2+}|Fe} = -0.42 \, V$ (in $, V$)

Which of the following is correct as a Nernst equation for the given electrochemical cell ?
$Mg_{(s)}|Mg_{(aq)}^{2+}(0.1 \ M)||Cl_{(aq)}^{-}(0.1 \ M)|Cl_{2_{(g)}}(1 \ bar)|Pt_{(s)}$