Standard cell potential and spontaneity

What is the standard cell potential, $E^\ominus_\text{cell}$, of the following cell? $\ce{Pb^2+(aq) + 2e- <=> Pb(s)}$ $E^\ominus = -0.13\ \mathrm{V}$ $\ce{Zn^2+(aq) + 2e- <=> Zn(s)}$ $E^\ominus = -0.76\ \mathrm{V}$ A. $-0.89\ \mathrm{V}$ B. $-0.63\ \mathrm{V}$…

The table shows standard electrode potentials for three metals. Half-equation $E^\ominus$ / V $\ce{Mn^2+(aq) + 2e- <=> Mn(s)}$ −1.18 $\ce{Cr^3+(aq) + 3e- <=> Cr(s)}$ −0.74 $\ce{Cd^2+(aq) + 2e- <=> Cd(s)}$ −0.40 Which combination undergoes a spontaneous…

Using section 19 of the data booklet, predict and explain what would be observed if zinc and silver metals were each added to a separate sample of blue copper(II) sulfate solution. Metal added Zn Ag Observations

The electrode potential, $E$, of the $\ce{Sn^4+}/\ce{Sn^2+}$ half-cell is not fixed: it depends on the concentrations of the two tin ions, as given by the equation: $E = 0.15 + \dfrac{RT}{2F}\ln\dfrac{[\ce{Sn^4+}]}{[\ce{Sn^2+}]}$ Determine the electrode…

(i) In the nickel–metal hydride (NiMH) rechargeable battery the negative electrode is a metal alloy, M, that absorbs hydrogen. The two electrode reactions during discharge are shown below. $\ce{MH(s) + OH-(aq) <=> M(s) + H2O(l) + e-}$…

For a different pair of half-cells, the standard Gibbs energy change, $\Delta G^\ominus$, works out to $-370.6\ \mathrm{kJ\,mol^{-1}}$, with a single electron transferred between the electrodes in the cell reaction. Deduce what these two half-cells are. Use…

A voltaic cell is made by connecting a manganese half-cell ($\ce{Mn(s)}$ in $\ce{Mn^2+(aq)}$) and a tin half-cell ($\ce{Sn(s)}$ in $\ce{Sn^2+(aq)}$) under standard conditions. $\ce{Mn^2+(aq) + 2e- <=> Mn(s)}$ $E^\ominus = -1.18\ \mathrm{V}$…