Quick questions on Electrochemistry, electrode potentials and electrolysis: Singapore A-Level H2 Chemistry

The standard electrode potential $E^{\circ}$ of a half-cell is its potential measured under standard conditions ($298$ K, $1$ bar, $1$ mol dm$^{-3}$ ion concentration) relative to the standard hydrogen electrode, which is defined as $0.00$ V. A more positive $E^{\circ}$ means the species is more readily reduced (a stronger oxidising agent).

When two half-cells are connected, the cell potential is:

Changing concentrations shifts an electrode potential (qualitatively, by Le Chatelier on the half-equation):

Read the half-equation: $\text{Al}^{3+} + 3e^-$ needs three electrons per aluminium, $\text{Cu}^{2+} + 2e^-$ needs two.

Define standard electrode potential. [2 marks]

Given $E^{\circ}(\text{Ag}^+/\text{Ag}) = +0.80$ V and $E^{\circ}(\text{Cu}^{2+}/\text{Cu}) = +0.34$ V, calculate $E^{\circ}_{cell}$ and state which metal dissolves. [3 marks]

A current of $2.00$ A flows for $30.0$ minutes through aqueous copper(II) sulfate. Calculate the mass of copper deposited. ($F = 96500$, Ar(Cu) = $63.5$.)