At 298 K, the following reaction takes place at the hydrogen electrode: testbook.com H+(aq) + e− → 12H2(g) (1 bar) If the solution pH is 10.0, what is the hydrogen electrode potential in volts? (Take 2.303 RTF = 0.06 V)

Calculate the oxidation potential (emf) of the given half-cell: Pt(s) | H2(g, 2 atm) | HCl(aq, 0.02 M) Given E°H2/H+ = 0 V, 2.303 RTF = 0.059, and log 2 = 0.3010.

A solution of copper sulphate is electrolysed for 10 minutes with a current of 1.5 amperes. The mass of copper deposited at cathode is: (Given: Molar mass of Cu = 63 g mol-1, 1 F = 96487 C mol-1)