Using the standard reduction potential data given below at 298 K, find out the strongest reducing agent among the choices: E° (Cr2O72-/Cr3+) = +1.33 V E° (Cl2/Cl-) = +1.36 V E° (MnO4-/Mn2+) = +1.51 V E° (Cr3+/Cr) = -0.74 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)