Depict the galvanic cell in which the reactionZn(s) + 2Ag+(aq) —-> 7M2+(aq) + 2Ag (s) takes place. Further show:(i) Which of the electrode is negatively charged?(ii) The carriers of the current in the cell.(iii) Individual reaction at each electrode.

The given reaction is a redox reaction that can be split into two half-reactions:

1. Oxidation half-reaction: Zn(s) —> Zn2+(aq) + 2e-
2. Reduction half-reaction: 2Ag+(aq) + 2e- —> 2Ag(s)

The galvanic cell can be depicted as follows:

• The anode is the electrode where oxidation takes place. Here, it is the zinc electrode. Zinc loses electrons and gets oxidized to Zn2+. So, the anode is made of zinc (Zn).
• The cathode is the electrode where reduction takes place. Here, it is the silver electrode. Silver ions gain electrons and get reduced to Ag. So, the cathode is made of silver (Ag).
• The salt bridge can be a U-tube filled with a solution of a salt such as KNO3. It allows the flow of ions and completes the circuit.

(i) The electrode that is negatively charged is the anode. In this case, it is the zinc electrode because it is where oxidation is taking place and electrons are being produced.

(ii) The carriers of the current in the cell are ions and electrons. In the external circuit (the wire connecting the electrodes), the current is carried by electrons. In the internal circuit (the electrolyte solutions and the salt bridge), the current is carried by ions. Cations (like Zn2+ and K+) move towards the cathode and anions (like NO3-) move towards the anode.

(iii) The individual reactions at each electrode are:

• At the anode (Zn electrode): Zn(s) —> Zn2+(aq) + 2e- (oxidation)
• At the cathode (Ag electrode): 2Ag+(aq) + 2e- —> 2Ag(s) (reduction)