For the half-cell Zn^{2+} | Zn,the standard e | vedclass

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(B) The cell reaction is: $Zn_{(s)} + 2H^{+}_{(aq)} \rightarrow Zn^{2+}_{(aq)} + H_{2(g)}$.The standard cell potential is given by $E^{\circ}_{cell} =

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$+0.76$

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(B) The cell reaction is: $Zn_{(s)} + 2H^{+}_{(aq)} \rightarrow Zn^{2+}_{(aq)} + H_{2(g)}$.The standard cell potential is given by $E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode}$.Here,the cathode is the Standard Hydrogen Electrode $(SHE)$,so $E^{\circ}_{cathode} = 0.00 \ V$.The anode is the $Zn^{2+}/Zn$ electrode,so $E^{\circ}_{anode} = -0.76 \ V$.Therefore,$E^{\circ}_{cell} = 0.00 \ V - (-0.76 \ V) = +0.76 \ V$.

For the half-cell $Zn^{2+} | Zn$,the standard electrode potential $E^{\circ}$ is $-0.76 \ V$. What is the $e.m.f.$ of the cell $Zn_{(s)} | Zn^{2+}_{(aq)} (1 \ M) || 2H^{+}_{(aq)} (1 \ M) | H_{2(g)} (1 \ atm)$ in $V$?

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