The oxidation potentials of Zn, Cu, Ag, H_2 a | vedclass

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Question

(B) The cell voltage $(E_{cell})$ is calculated as $E_{cell} = E_{ox} + E_{red}$.For a reaction $A + B^{n+} \rightarrow A^{n+} + B$,$E_{cell} = E_{ox}

Vedclass · Accepted Answer

$Zn + 2Ag^{+} \rightarrow 2Ag + Zn^{2+}$

Vedclass · Answer

(B) The cell voltage $(E_{cell})$ is calculated as $E_{cell} = E_{ox} + E_{red}$.For a reaction $A + B^{n+} \rightarrow A^{n+} + B$,$E_{cell} = E_{ox}(A) + E_{red}(B^{n+})$.Given oxidation potentials $(E_{ox})$: $Zn = 0.76 \ V, Cu = -0.34 \ V, Ag = -0.80 \ V, H_2 = 0 \ V, Ni = 0.25 \ V$.Reduction potentials $(E_{red} = -E_{ox})$: $Cu^{2+} = 0.34 \ V, Ag^{+} = 0.80 \ V, H^{+} = 0 \ V, Ni^{2+} = -0.25 \ V$.$(A)$ $Zn + Cu^{2+} \rightarrow Zn^{2+} + Cu$: $E_{cell} = 0.76 + 0.34 = 1.10 \ V$.$(B)$ $Zn + 2Ag^{+} \rightarrow Zn^{2+} + 2Ag$: $E_{cell} = 0.76 + 0.80 = 1.56 \ V$.$(C)$ $H_2 + Cu^{2+} \rightarrow 2H^{+} + Cu$: $E_{cell} = 0 + 0.34 = 0.34 \ V$.$(D)$ $H_2 + Ni^{2+} \rightarrow 2H^{+} + Ni$: $E_{cell} = 0 + (-0.25) = -0.25 \ V$.The maximum voltage is $1.56 \ V$ for option $B$.

The oxidation potentials of $Zn, Cu, Ag, H_2$ and $Ni$ are $0.76, -0.34, -0.80, 0$ and $0.25 \ V$ respectively. Which reaction provides the maximum voltage?

Similar Questions

If the emf of the cell $Cu(s) | Cu^{2+}(1M) || Ag^+(1M) | Ag(s)$ is $0.463 \text{ V}$ at $25^{\circ} \text{C}$ and the standard electrode potential of the $Cu$ electrode is $0.337 \text{ V}$, find the standard electrode potential of the $Ag$ electrode. (in $\text{ V}$)

The $E^{\ominus}$ for $Cl_{2}/Cl^{-}$ is $+1.36 \ V,$ for $I_{2}/I^{-}$ is $+0.53 \ V,$ for $Ag^{+}/Ag$ is $+0.79 \ V,$ $Na^{+}/Na$ is $-2.71 \ V$ and for $Li^{+}/Li$ is $-3.04 \ V.$ Arrange the following ionic species in decreasing order of reducing strength: $I^{-}, Ag, Cl^{-}, Li, Na$

$E^{\circ}$ of $Cu$ is $+0.34 \ V$ while that of $Zn$ is $-0.76 \ V$. Explain.

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

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