The standard oxidation potentials for the hal | vedclass

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(B) The given reactions are oxidation half-reactions. The standard reduction potentials $(E^o_{red})$ are the negative of the standard oxidation poten

Vedclass · Accepted Answer

$+0.35$

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(B) The given reactions are oxidation half-reactions. The standard reduction potentials $(E^o_{red})$ are the negative of the standard oxidation potentials $(E^o_{ox})$.$E^o_{red}(Zn^{2+}/Zn) = -0.76 \ V$$E^o_{red}(Fe^{2+}/Fe) = -0.41 \ V$In the cell reaction $Fe^{2+} + Zn 	o Zn^{2+} + Fe$,$Zn$ is oxidized (anode) and $Fe^{2+}$ is reduced (cathode).$E^o_{cell} = E^o_{cathode} - E^o_{anode}$$E^o_{cell} = E^o_{red}(Fe^{2+}/Fe) - E^o_{red}(Zn^{2+}/Zn)$$E^o_{cell} = -0.41 \ V - (-0.76 \ V)$$E^o_{cell} = -0.41 \ V + 0.76 \ V = +0.35 \ V$.

The standard oxidation potentials for the half-reactions are given as $Zn \to Zn^{2+} + 2e^{-}; E^o = +0.76 \ V$ and $Fe \to Fe^{2+} + 2e^{-}; E^o = +0.41 \ V$. The $EMF$ for the cell reaction $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.

Similar Questions

Given $E^{0}_{Fe^{2+}|Fe} = -0.441 \, V$ and $E^{0}_{Fe^{3+}|Fe^{2+}} = 0.771 \, V$,calculate the standard $EMF$ for the reaction $Fe + 2Fe^{3+} \rightarrow 3Fe^{2+}$ in $V$.

Identify which of the following cell reactions is spontaneous under standard state conditions.

In a cell reaction
$Cu_{(s)} + 2Ag^{+}_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)}$
$E_{cell}^o = + 0.46 \ V$.
If the concentration of $Cu^{2+}$ ions is doubled,then $E_{cell}^o$ will be

On the basis of the following $E^o$ values,the strongest oxidizing agent is:
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-; E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-; E^o = -0.77 \ V$

What is the procedure to determine the cell potential?

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