The figure shows one cell of a lead storage battery. The negative plate is lead and the positive plate is lead dioxide, both in sulfuric acid. On discharge the overall reaction is $\text{Pb}(s) + \text{PbO}_2(s) + 2\text{H}_2\text{SO}_4(aq) \rightarrow 2\text{PbSO}_4(s) + 2\text{H}_2\text{O}(l)$, and the lead sulfate sticks to the plates. The cell holds $500\ \text{g}$ of acid that is $38.0$ per cent $\text{H}_2\text{SO}_4$ by mass. It now delivers a steady current of $2.00\ \text{A}$ for $5.00\ \text{h}$. Take $F = 96487\ \text{C mol}^{-1}$ and molar masses in $\text{g mol}^{-1}$: $\text{H}_2\text{SO}_4$ 98.1, $\text{H}_2\text{O}$ 18.0, $\text{SO}_4$ 96.1 and $\text{SO}_2$ 64.1. Which of the following statements are correct?

Fig. 1: One cell of a lead storage battery. A container holds sulfuric acid, 38.0 per cent by mass. A lead plate is marked as the negative terminal and a lead dioxide plate as the positive terminal. Wires from the plates run through an ammeter reading 2.00 A to a lamp.