(B) For a galvanic cell,the standard $emf$ $(E^o_{cell})$ is calculated as: $E^o_{cell} = E^o_{cathode} - E^o_{anode}$.Since $Zn$ has a more negative

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(B) For a galvanic cell,the standard $emf$ $(E^o_{cell})$ is calculated as: $E^o_{cell} = E^o_{cathode} - E^o_{anode}$.Since $Zn$ has a more negative reduction potential than $Ni$,$Zn$ acts as the anode and $Ni$ acts as the cathode.$E^o_{cathode} = E^o_{Ni^{2+}/Ni} = -0.25 \ V$.$E^o_{anode} = E^o_{Zn^{2+}/Zn} = -0.76 \ V$.$E^o_{cell} = (-0.25 \ V) - (-0.76 \ V) = -0.25 \ V + 0.76 \ V = +0.51 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Easy

The standard electrode potentials of two half-cells are given as: $Ni^{2+}_{(aq)} + 2e^{-} \rightarrow Ni_{(s)}$; $E^o = -0.25 \ V$ and $Zn^{2+}_{(aq)} + 2e^{-} \rightarrow Zn_{(s)}$; $E^o = -0.76 \ V$. What is the standard $emf$ of the cell formed by connecting these two half-cells in $volt$?

A
$-1.01$
B
$+0.51$
C
$+1.01$
D
$-0.51$

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Class 12

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Electrochemistry

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Electrode potential and ECell

Which of the following will have a standard oxidation potential less than $SHE$?

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$K,$ $Ca,$ and $Li$ metals may be arranged in the increasing order of their standard electrode potentials as

Medium

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$A$ cell is constructed by dipping a copper rod in $1\,M\,CuSO_4$ solution and a nickel rod in $1\,M\,NiSO_4$ solution. The standard reduction potentials of copper and nickel electrodes are $+0.34\,V$ and $-0.25\,V$ respectively. Calculate the $EMF$ of the cell. (in $,V$)

Easy

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From the given values,which one is a strong oxidizing agent?
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$

Easy

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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

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The standard electrode potentials of two half-cells are given as: $Ni^{2+}_{(aq)} + 2e^{-} \rightarrow Ni_{(s)}$; $E^o = -0.25 \ V$ and $Zn^{2+}_{(aq)} + 2e^{-} \rightarrow Zn_{(s)}$; $E^o = -0.76 \ V$. What is the standard $emf$ of the cell formed by connecting these two half-cells in $volt$?

Similar Questions

Which of the following will have a standard oxidation potential less than $SHE$?

$K,$ $Ca,$ and $Li$ metals may be arranged in the increasing order of their standard electrode potentials as

$A$ cell is constructed by dipping a copper rod in $1\,M\,CuSO_4$ solution and a nickel rod in $1\,M\,NiSO_4$ solution. The standard reduction potentials of copper and nickel electrodes are $+0.34\,V$ and $-0.25\,V$ respectively. Calculate the $EMF$ of the cell. (in $,V$)

From the given values,which one is a strong oxidizing agent?$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$

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

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From the given values,which one is a strong oxidizing agent?
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$

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