. Choose the correct line notation for the following galvanic cell reaction:2Al(s) + 3Cu+2(aq) → Al+3(aq) + 3Cu(s)Line Notation: Cu2+(aq) | Cu(s) || Al(s) | Al3+(aq)Al3+(aq) | Al(s) || Cu(s) | Cu2+(aq)Al(s) | Al3+(aq) || Cu2+(aq) | Cu(s)

Which reaction occurs at the cathode in an electrochemical cell?A.Cu(s) Cu2+(aq) + 2e-B.Cu2+(aq) + 2e- Cu(s)C.Cu(s) + 2H+(aq) Cu2+(aq) + H2(g)D.Cu2+(aq) + H2(g) Cu(s) + 2H+(aq)

What are the half-reactions for a galvanic cell with aluminum and gold electrodes?A.Al(s) Al3+(aq) + 3e- and Au+(aq) + e- Au(s)B.Al(s) Al3+(aq) + 3e- and Au(s) Au+(aq) + e-C.Al3+(aq) + 3e- Al(s) and Au+(aq) + e- Au(s)D.Al3+(aq) + 3e- Al(s) and Au(s) Au+(aq) + e-

What is the standard cell notation for an electrolytic cell with aluminum and gold electrodes?A.Au+(aq) | Au(s) || Al(s) | Al3+(aq)B.Al3+(aq) | Al(s) || Au(s) | Au+(aq)C.Al(s) | Al3+(aq) || Au+(aq) | Au(s)D.Au(s) | Au+(aq) || Al3+(aq) | Al(s)SUBMITarrow_backPREVIOUS

To write the shorthand notation for the given galvanic cell, we need to follow these steps: 1. **Identify the anode and cathode reactions:** - **Anode (oxidation):** Lead (Pb) is oxidized to lead ions (Pb²⁺). \[ \text{Pb(s)} \rightarrow \text{Pb}^{2+}(\text{aq}) + 2\text{e}^- \] - **Cathode (reduction):** Ferric ions (Fe³⁺) are reduced to ferrous ions (Fe²⁺). \[ \text{Fe}^{3+}(\text{aq}) + \text{e}^- \rightarrow \text{Fe}^{2+}(\text{aq}) \] 2. **Write the cell notation:** - The anode (oxidation) half-cell is written on the left. - The cathode (reduction) half-cell is written on the right. - A single vertical line (|) separates different phases within the same half-cell. - A double vertical line (||) represents the salt bridge between the two half-cells. Given the reactions: - Anode: \(\text{Pb(s)} \rightarrow \text{Pb}^{2+}(\text{aq}) + 2\text{e}^-\) - Cathode: \(\text{Fe}^{3+}(\text{aq}) + \text{e}^- \rightarrow \text{Fe}^{2+}(\text{aq})\) The shorthand notation for the galvanic cell is: \[ \text{Pb(s)} | \text{Pb}^{2+}(\text{aq}) || \text{Fe}^{3+}(\text{aq}), \text{Fe}^{2+}(\text{aq}) | \text{Pt(s)} \] Here: - \(\text{Pb(s)}\) is the solid lead electrode. - \(\text{Pb}^{2+}(\text{aq})\) is the lead ion in solution. - \(\text{Fe}^{3+}(\text{aq})\) and \(\text{Fe}^{2+}(\text{aq})\) are the ferric and ferrous ions in solution. - \(\text{Pt(s)}\) is the platinum electrode used as an inert conductor for the cathode reaction

For the reactionZn(s) + Cu+2(0.1 M) → Zn+2(1 M) + Cu(s)taking place in a cell,  is 1.10 volt.ECell for the cell will be Given : 2.14 volt1.80 volt1.07 volt0.82 volt