Final answer:
In this battery, Cu is oxidized to Cu2+ ions, while Ag+ ions are reduced to Ag solid. The standard cell potential is +0.46 V. The direction of electron flow is from the Cu anode to the Ag cathode. Increasing the concentration of Ag+ ions will decrease the cell potential.
Step-by-step explanation:
In this battery, the copper (Cu) solid is oxidized to produce Cu2+ ions, while silver ions (Ag+) are reduced to form solid silver (Ag). Therefore, the oxidized species is Cu and the reduced species is Ag+.
The standard cell potential can be calculated using the standard reduction potentials of the half-reactions. The reduction potential of Cu2+ + 2e- → Cu is +0.34 V, and the reduction potential of Ag+ + e- → Ag is +0.80 V. The standard cell potential (E°cell) is the difference between these two reduction potentials: E°cell = +0.80 V - (+0.34 V) = +0.46 V.
The direction of electron flow in the external circuit is from the anode (Cu) to the cathode (Ag). This is because oxidation occurs at the anode, where electrons are released, while reduction occurs at the cathode, where electrons are gained.
If the concentration of Ag+ ions is increased, the cell potential will decrease. According to Le Chatelier's principle, increasing the concentration of Ag+ ions on the right (reduction) side of the cell will shift the equilibrium towards the left (oxidation) side, resulting in a decrease in cell potential.