List of top Metallurgical Thermodynamics Questions on Electrochemistry asked in GATE MT

Copper is being electrodeposited from a CuSO\(_4\) bath onto a stainless steel cathode of total surface area of 2 m\(^2\) in an electrolytic cell operated at a current density of 200 A m\(^{-2}\) with a current efficiency of 90%. The mass of copper deposited in 24 h is _________ kg (rounded off to two decimal places). Given: Faraday's constant = 96500 C mol\(^{-1}\), Atomic mass of copper = 63.5 g mol\(^{-1}\).
Consider the following cell reaction: Mg + Cd$^{2+}$ ⇌ Mg$^{2+}$ + Cd The standard Gibbs free energy change for the reaction is ........... kJ (rounded off to an integer). Given: Standard oxidation potentials with respect to standard hydrogen electrode are: Mg ⇌ Mg$^{2+}$ + 2e$^-$, E° = 2.37 V
Cd ⇌ Cd$^{2+}$ + 2e$^-$, E° = 0.403 V
Faraday's constant = 96500 C mol$^{-1}$

Copper is being electrodeposited from a CuSO\(_4\) bath onto a stainless steel cathode of total surface area of 2 m\(^2\) in an electrolytic cell operated at a current density of 200 A m\(^{-2}\) with a current efficiency of 90%. The mass of copper deposited in 24 h is _________ kg (rounded off to two decimal places). Given: Faraday's constant = 96500 C mol\(^{-1}\), Atomic mass of copper = 63.5 g mol\(^{-1}\).