(C) The standard cell potential is calculated using the formula: $E^o_{cell} = E^o_{cathode} - E^o_{anode}$.In the given cell $Zn | Zn^{2+} || Cu^{2+}

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(C) The standard cell potential is calculated using the formula: $E^o_{cell} = E^o_{cathode} - E^o_{anode}$.In the given cell $Zn | Zn^{2+} || Cu^{2+} | Cu$,the $Cu^{2+} | Cu$ electrode acts as the cathode and $Zn^{2+} | Zn$ acts as the anode.Given $E^o_{cathode} = E^o_{Cu^{2+} | Cu} = +0.34 \ V$ and $E^o_{anode} = E^o_{Zn^{2+} | Zn} = -0.76 \ V$.Substituting these values: $E^o_{cell} = 0.34 \ V - (-0.76 \ V) = 0.34 + 0.76 = 1.10 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

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What is the standard cell potential for the cell $Zn | Zn^{2+} (1M) || Cu^{2+} (1M) | Cu$? Given $E^o$ for $Zn^{2+} | Zn = -0.76 \ V$ and $E^o$ for $Cu^{2+} | Cu = +0.34 \ V$.

AIIMS 1980 All AIIMS

A
$-0.76 + (-0.34) = -0.42 \ V$
B
$-0.34 + 0.76 = +0.42 \ V$
C
$0.34 - (-0.76) = 1.10 \ V$
D
$-0.76 - (+0.34) = -1.10 \ V$

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Electrode potential and ECell

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AIIMS 1980 Paper All AIIMS years →

The cell potential of the given cell is $0.34 \, V$. Write the cell reaction and calculate $E^o_{Cu^{2+}|Cu}$.
$Pt_{(s)} \mid H_{2(g)} (1 \, bar) \mid H^+_{(1 \, M)} \parallel Cu^{2+}_{(1 \, M)} \mid Cu_{(s)}$

Medium

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Calculate the standard cell potential for a cell having the following reaction: $2 Al_{(s)} + 3 Ni^{2+} \rightarrow 2 Al^{3+} + 3 Ni_{(s)}$ given that $E_{Ni^{2+}/Ni}^{\circ} = -0.25 \ V$ and $E_{Al^{3+}/Al}^{\circ} = -1.66 \ V$. (in $V$)

EasyMHT CET 2022

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Based on the given standard electrode potentials,identify the metal that can be displaced from its salt solution by all other metals listed.
$E^o Zn^{2+}/Zn = -0.76 \ V, E^o Cu^{2+}/Cu = +0.34 \ V$
$E^o Ag^+/Ag = +0.80 \ V, E^o Co^{2+}/Co = -0.28 \ V$

Medium

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Given that $E_{O_2/H_2O}^o = +1.23 \ V$; $E_{S_2O_8^{2-}/SO_4^{2-}}^o = 2.05 \ V$; $E_{Br_2/Br^-}^o = +1.09 \ V$; $E_{Au^{3+}/Au}^o = 1.4 \ V$. The strongest oxidizing agent is

DifficultJEE MAIN 2019

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The standard electrode potentials of $Zn^{2+}/Zn$ and $Ag^{+}/Ag$ are $-0.763 \ V$ and $+0.799 \ V$ respectively. The standard potential of the cell is ............ $V$.

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What is the standard cell potential for the cell $Zn | Zn^{2+} (1M) || Cu^{2+} (1M) | Cu$? Given $E^o$ for $Zn^{2+} | Zn = -0.76 \ V$ and $E^o$ for $Cu^{2+} | Cu = +0.34 \ V$.

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The cell potential of the given cell is $0.34 \, V$. Write the cell reaction and calculate $E^o_{Cu^{2+}|Cu}$.$Pt_{(s)} \mid H_{2(g)} (1 \, bar) \mid H^+_{(1 \, M)} \parallel Cu^{2+}_{(1 \, M)} \mid Cu_{(s)}$

Calculate the standard cell potential for a cell having the following reaction: $2 Al_{(s)} + 3 Ni^{2+} \rightarrow 2 Al^{3+} + 3 Ni_{(s)}$ given that $E_{Ni^{2+}/Ni}^{\circ} = -0.25 \ V$ and $E_{Al^{3+}/Al}^{\circ} = -1.66 \ V$. (in $V$)

Based on the given standard electrode potentials,identify the metal that can be displaced from its salt solution by all other metals listed.$E^o Zn^{2+}/Zn = -0.76 \ V, E^o Cu^{2+}/Cu = +0.34 \ V$$E^o Ag^+/Ag = +0.80 \ V, E^o Co^{2+}/Co = -0.28 \ V$

Given that $E_{O_2/H_2O}^o = +1.23 \ V$; $E_{S_2O_8^{2-}/SO_4^{2-}}^o = 2.05 \ V$; $E_{Br_2/Br^-}^o = +1.09 \ V$; $E_{Au^{3+}/Au}^o = 1.4 \ V$. The strongest oxidizing agent is

The standard electrode potentials of $Zn^{2+}/Zn$ and $Ag^{+}/Ag$ are $-0.763 \ V$ and $+0.799 \ V$ respectively. The standard potential of the cell is ............ $V$.

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The cell potential of the given cell is $0.34 \, V$. Write the cell reaction and calculate $E^o_{Cu^{2+}|Cu}$.
$Pt_{(s)} \mid H_{2(g)} (1 \, bar) \mid H^+_{(1 \, M)} \parallel Cu^{2+}_{(1 \, M)} \mid Cu_{(s)}$

Based on the given standard electrode potentials,identify the metal that can be displaced from its salt solution by all other metals listed.
$E^o Zn^{2+}/Zn = -0.76 \ V, E^o Cu^{2+}/Cu = +0.34 \ V$
$E^o Ag^+/Ag = +0.80 \ V, E^o Co^{2+}/Co = -0.28 \ V$