ElectrochemistryHard
Question
For a cell reaction involving a two-electron change, the standard EMF of the cell is found to be 0.295 V at 25°C. The equilibrium constant of the reaction at 25°C will be
Options
A.1 × 1010
B.1 × 10−10
C.29.5 × 10−2
D.2 × 1010
Solution
$E_{cell}^{o} = \frac{0.059}{n}.\log K_{eq} \Rightarrow 0.295 = \frac{0.059}{2}.\log K_{eq}$
$\therefore K_{eq} = 10^{10}$
Create a free account to view solution
View Solution FreeMore Electrochemistry Questions
Faraday’s law of electrolysis fails when...The standard reduction potentials at 25°C of Li+|Li, Ba2+|Ba, Na+|Na and Mg2+|Mg are −3.05, −2.73, −2.71 and −2.37 V, re...The reaction, H2(g) + AgCl(s) → H+ (aq) + Cl- (aq) + Ag(s) occurs in the galvanic cell :...The molar conductance of a strong electrolyte at infinite dilution...Which Shows electrical conductance ?...