Given the standard potential for the following half-cell reaction at 298 K,
Cu⁺(aq) + e^- → Cu(s); E° = 0.52 V
Cu²⁺(aq) + e^- → Cu⁺(aq); E° = 0.16 V
Calculate the ΔG° (kJ) for the reaction, [2Cu⁺(aq) → Cu(s) + Cu²⁺]

For the concentration cell, M|M⁺ (aq, 0.01 mol/dm³)| |M⁺ (aq), 0.1 mol/dm³|M the EMF (E) of the cell at a temperature (T) equals

A. $$2.303\frac{{RT}}{F}$$

B. $$ - 2.303\frac{{RT}}{F}$$

C. $$E_{{M^ + }|m}^ \circ + 2.303\frac{{RT}}{F}$$

D. $$E_{{M^ + }|m}^ \circ - 2.303\frac{{RT}}{F}$$

The activity of water at 11 bar and 298 K is

A. 1.101

B. 1.007

C. 0.998

D. 0.898

Given that E°(Fe³⁺, Fe) = -0.4 V and E°(Fe²⁺, Fe) = -0.44 V, the value of E°(Fe³⁺, Fe²⁺) is

A. 0.76V

B. -0.40 V

C. -0.76 V

D. 0.40 V

According to the Debye-Huckel limiting law, if the concentration of a dilute aqueous solution of KCl is increased 4-fold, the value of In γ_z (γ_z is the molar mean ionic activity coefficient) will

A. decrease by a factor of 2

B. increase by a factor of 2

C. decrease by a factor of 4

D. increase by a factor of 4