The oxidation potentials of the following hal | vedclass

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(B) The given reactions are oxidation half-reactions:$Zn 	o Zn^{2+} + 2e^-; E^o_{ox} = 0.76 \, V$$Fe 	o Fe^{2+} + 2e^-; E^o_{ox} = 0.44 \, V$For the

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$+0.32 \, V$

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(B) The given reactions are oxidation half-reactions:$Zn 	o Zn^{2+} + 2e^-; E^o_{ox} = 0.76 \, V$$Fe 	o Fe^{2+} + 2e^-; E^o_{ox} = 0.44 \, V$For the cell reaction $Fe^{2+} + Zn 	o Zn^{2+} + Fe$,the oxidation occurs at the $Zn$ electrode (anode) and reduction occurs at the $Fe$ electrode (cathode).$E^o_{cell} = E^o_{cathode(red)} - E^o_{anode(red)}$Since $E^o_{red} = -E^o_{ox}$:$E^o_{cathode(red)} = -E^o(Fe 	o Fe^{2+}) = -0.44 \, V$$E^o_{anode(red)} = -E^o(Zn 	o Zn^{2+}) = -0.76 \, V$$E^o_{cell} = -0.44 - (-0.76) = -0.44 + 0.76 = +0.32 \, V$.

Element	$M^{3+}/M$	$M^{+}/M$
$Al$	$-1.66$	$+0.55$
$Tl$	$+1.26$	$-0.34$

The oxidation potentials of the following half-cell reactions are given:
$Zn \to Zn^{2+} + 2e^-; E^o = 0.76 \, V$
$Fe \to Fe^{2+} + 2e^-; E^o = 0.44 \, V$
What will be the $EMF$ of the cell whose cell reaction is:
$Fe^{2+}_{(aq)} + Zn \to Zn^{2+}_{(aq)} + Fe$

Similar Questions

Consider the following standard electrode potentials ($E^0$ in volts) in aqueous solution. Based on this data,which of the following statements is correct?
Element $M^{3+}/M$ $M^{+}/M$
$Al$ $-1.66$ $+0.55$
$Tl$ $+1.26$ $-0.34$

Given electrode potentials:
$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = 0.771 \, V$
$I_2 + 2e^- \to 2I^-$; $E^o = 0.536 \, V$
$E^o_{\text{cell}}$ for the cell reaction
$2Fe^{3+} + 2I^- \to 2Fe^{2+} + I_2$ is:

If the standard reduction potentials of $Zn$, $Ni$, and $Fe$ are $-0.76 \text{ V}$, $-0.23 \text{ V}$, and $-0.44 \text{ V}$ respectively, determine the electrodes $X$ and $Y$ for the reaction $X(s) + Y^{+2}(aq) \rightarrow X^{+2}(aq) + Y(s)$ to be spontaneous.

Which of the following metals cannot displace $H_2$ from acids or $H_2O$ from its compounds?

For the reaction taking place in the cell:
$Pt_{(s)} | H_{2(g)} | H^{+}_{(aq)} || Ag^{+}_{(aq)} | Ag_{(s)}$
$E_{Cell}^0 = +0.5332 \ V$.
The value of $\Delta_f G^0$ in $kJ \ mol^{-1}$ (nearest integer) is:

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The oxidation potentials of the following half-cell reactions are given:$Zn \to Zn^{2+} + 2e^-; E^o = 0.76 \, V$$Fe \to Fe^{2+} + 2e^-; E^o = 0.44 \, V$What will be the $EMF$ of the cell whose cell reaction is:$Fe^{2+}_{(aq)} + Zn \to Zn^{2+}_{(aq)} + Fe$