Given the equilibrium constant: K C of the reaction: Cu(s) + 2Ag⁺ (aq) → Cu²⁺ (aq) + 2Ag(s) is 10 × 10¹⁵, calculate the E cell ⁰ of this reaciton at 298 K [2.303 RT/F at 298 K = 0.059V]

Redox Reactions and Electrochemistry: JEE Main 2019 Chemistry question

JEE Main 2019 · 11 Jan, Evening shift · Q990

JEE Main 201911 Jan, Evening shiftChemistryMediumRedox Reactions and Electrochemistry138× since 2002

Given the equilibrium constant: K_C of the reaction : Cu(s) + 2Ag⁺ (aq)

\to

Cu²⁺ (aq) + 2Ag(s) is 10

\times

10¹⁵, calculate the E

_{cell}^0

of this reaciton at 298 K [2.303

{{RT} \over F}

at 298 K = 0.059V]