When Cu reacts with AgNO₃ solution, the reaction takes place is:

• oxidation of Cu

• reduction of Cu

• oxidation of Ag

• reduction of NO${}_3^{-}$

For a cell involving one electron E°_cell = 0.59 V at 298 K, the equilibrium constant for the cell reaction is :[ Given that $\frac{2.303}{\mathrm{F}}= 0.059\mathrm{V} \mathrm{at} \mathrm{T} = 298 \mathrm{K}]$.

• 1.0 × 10⁵

• 1.0 × 10¹⁰

• 1.0 × 10³⁰

• 1.0 × 10²

413.

For the cell reaction

2Fe³⁺ (aq) +2l^-(aq) → 2Fe²⁺(aq) + I₂(aq)

E${}_{\mathrm{cell}}^{⊝}$= 0.24V at 298 K. The standard Gibbs energy (Δ_rG^Θ) of the cell reaction is:

[Given that Faraday constant F = 96500 C mol^–1]

• – 23.16 kJ mol^–1

• 46.32 kJ mol^-1

• 23.16 kJ mol^-1

• - 46.32 kJ mol^-1