Define standard cell potential, $E^\ominus_{\text{cell}}$. State the standard conditions in your response.
Draw a labelled diagram of this electrochemical cell. Include all necessary substances and the relevant apparatus required to measure the $E^\ominus_{\text{cell}}$. It is not necessary to state the conditions used.
State the charge carriers that transfer current through the solutions and through the wire. The solutions __________ The wire __________
The standard electrode potential, $E^\ominus$, for the $\text{Zn}^{2+}(\text{aq})/\text{Zn}(\text{s})$ electrode is $-0.76\text{ V}$. Water is added to a standard $\text{Zn}^{2+}(\text{aq})/\text{Zn}(\text{s})$ electrode. The new concentration of $\text{Zn}^{2+}(\text{aq})$ becomes $0.25\text{ mol dm}^{-3}$. Use the Nernst equation to work out the electrode potential, $E$, for this updated $\text{Zn}^{2+}(\text{aq})/\text{Zn}(\text{s})$ electrode.
An electrochemical cell has a $\text{ZnO}/\text{Zn}$ electrode and a $\text{MnO}_2/\text{Mn}_2\text{O}_3$ electrode in an alkaline electrolyte. The standard cell potential, $E^\circ_{\text{cell}}$, for this cell is $+1.47\,\text{V}$. The half-equation at each electrode when this cell is discharging is shown. $\text{Zn} + 2\text{OH}^- \rightarrow \text{ZnO} + \text{H}_2\text{O} + 2e^-$ $2\text{MnO}_2 + \text{H}_2\text{O} + 2e^- \rightarrow \text{Mn}_2\text{O}_3 + 2\text{OH}^-$ Use this information to determine the change in oxidation state of manganese when this cell is discharging. from ........................ to ........................
Write the equation for the overall reaction that occurs when this cell is discharging.
The $E^\circ$ for the $\text{ZnO}/\text{Zn}$ electrode is $-1.28\,\text{V}$. Calculate the standard electrode potential, $E^\circ$, for the $\text{MnO}_2/\text{Mn}_2\text{O}_3$ electrode.