The cathode in this cell and the maximum voltage produced by this cell, under standard conditions, are respectively A - VCE - SSCE Chemistry - Question 18 - 2012 - Paper 1

To determine the cathode and maximum voltage of the cell, we first need to understand the standard electrode potentials of the metals involved.

In electrochemical cells, the cathode is the electrode where reduction occurs. From standard reduction potential tables, we know:

• Silver (Ag) has a reduction potential of +0.80 V, which indicates it is a strong oxidizing agent.
• Zinc (Zn) has a lower reduction potential of -0.76 V, indicating it is a reducing agent.

Given these potentials, the silver electrode would act as the cathode, while zinc would act as the anode in the electrochemical cell.

Next, to find the maximum voltage of the cell, we calculate the difference between the reduction potential of the cathode (Ag) and the anode (Zn):

$\text{Cell Voltage} = E_{cathode} - E_{anode} = 0.80 V - (-0.76 V) = 0.80 V + 0.76 V = 1.56 V$

Thus, the maximum voltage produced by this cell is 1.56 V.