solution containing 0.15M Cu(2) at pH 4 is electrolysed for deposition of Cu. Oxygen evolves during the process at the anode at a partial pressure of 700 torr. The cell has a resistance of 3.5ohm and the temperature is 25 degree celsius. Calculate: 1. The theoretical potential needed to initiate deposition of Cu from this solution. 2. The IR drop associated with a current of 0.2 A in this cell.

1. Theoretical Potential Calculation:

The Nernst equation is used to calculate the theoretical potential needed to initiate the deposition of Cu from this solution. The equation is as follows:

E = E° - (RT/nF) * ln([Cu2+])

Where: E° is the standard reduction potential for the Cu2+/Cu couple, which is +0.34V. R is the universal gas constant, which is 8.314 J/(mol*K). T is the temperature in Kelvin, which is 25°C = 298.15K. n is the number of electrons transferred in the half-reaction, which is 2 for the Cu2+/Cu couple. F is Faraday's constant, which is 96485 C/mol. [Cu2+] is the concentration of Cu2+ ions, which is 0.15M.

Substituting these values into the Nernst equation gives:

E = 0.34V - (8.314 J/(mol*K) * 298.15K / (2 * 96485 C/mol)) * ln(0.15)

This will give you the theoretical potential needed to initiate the deposition of Cu from this solution.

2. IR Drop Calculation:

Ohm's law (V = IR) is used to calculate the IR drop associated with a current of 0.2 A in this cell. The resistance (R) is given as 3.5 ohms, and the current (I) is 0.2 A.

Substituting these values into Ohm's law gives:

V = 0.2 A * 3.5 ohms = 0.7 V

This is the IR drop associated with a current of 0.2 A in this cell.