Calculate the standard cell potential for the galvanic cell $Zn_{(s)} | Zn^{2+}_{(aq)} || Ag^{+}_{(aq)} | Ag_{(s)}$,given that $E^o_{Zn^{2+}/Zn} = -0.76 \ V$ and $E^o_{Ag^{+}/Ag} = +0.80 \ V$. (in $V$)

Four alkali metals $A$,$B$,$C$ and $D$ have standard electrode potentials of $-3.05 \ V$,$-1.66 \ V$,$-0.40 \ V$ and $0.80 \ V$ respectively. Which one will be the most reactive?

Why does copper not replace hydrogen from acids?

The standard electrode potential $(E^{\circ})$ values of $Al^{3+}/Al, Ag^{+}/Ag, K^{+}/K$ and $Cr^{3+}/Cr$ are $-1.66 \ V, 0.80 \ V, -2.93 \ V$ and $-0.74 \ V,$ respectively. The correct decreasing order of reducing power of the metal is:

Based on the given data,which is the strongest oxidizing agent? $E_{Li^+|Li}^o = -3.03 \ V$,$E_{Ba^{2+}|Ba}^o = -2.73 \ V$,$E_{Na^+|Na}^o = -2.71 \ V$,and $E_{Mg^{2+}|Mg}^o = -2.37 \ V$.

The standard electrode potential for the Daniell cell is $1.1 \, V$. Calculate the standard Gibbs energy for the reaction:
$Zn_{(s)} + Cu^{2+}_{(aq)} \rightarrow Zn^{2+}_{(aq)} + Cu_{(s)}$