An oxidation-reduction reaction in which
3 electrons are transferred has a $$\Delta $$Gº of 17.37 kJ mol^–1 at
25 ^oC. The value of E^o
cell (in V) is ______ × 10^–2.
(1 F = 96,500 C mol^–1)

An acidic solution of dichromate is electrolyzed for 8 minutes using 2A current. As per the following equation
Cr₂O₇^2- + 14H⁺ + 6e^– $$ \to $$ 2Cr³⁺ + 7H₂O
The amount of Cr³⁺ obtained was 0.104 g. The efficiency of the process(in%) is (Take : F = 96000 C, At. mass of chromium = 52) ______.

The photoelectric current from Na (Work function, w₀ = 2.3 eV) is stopped by the output voltage of the cell
Pt(s) | H₂ (g, 1 Bar) | HCl (aq., pH =1) | AgCl(s) | Ag(s).
The pH of aq. HCl required to stop the photoelectric current form K(w₀ = 2.25 eV), all other conditions remaining the same, is _______ $$ \times $$ 10^-2 (to the nearest integer).

Given, 2.303$${{RT} \over F}$$ = 0.06 V;
$$E_{AgCl|Ag|C{l^ - }}^0$$ = 0.22 V

For the disproportionation reaction
2Cu⁺(aq) ⇌ Cu(s) + Cu²⁺(aq) at 298 K. ln K
(where K is the equilibrium constant) is
___________ × 10^–1.
Given :
($$E_{C{u^{2 + }}/C{u^ + }}^0 = 0.16V$$
$$E_{C{u^ + }/Cu}^0 = 0.52V$$
$${{RT} \over F} = 0.025$$)