Jee Main
Electrochemistry
JEE Main 2021 (Online) 31st August Morning Shift
INTEGER+4 / -12021
Consider the following cell reaction :
\(C{d_{(s)}} + H{g_2}S{O_{4(s)}} + {9 \over 5}{H_2}{O_{(l)}}\) \(\rightleftharpoons\) \(CdS{O_4}.{9 \over 5}{H_2}{O_{(s)}} + 2H{g_{(l)}}\)
The value of \(E_{cell}^0\) is 4.315 V at 25\(^\circ\)C. If \(\Delta\)H\(^\circ\) = \(-\)825.2 kJ mol\(-\)1, the standard entropy change \(\Delta\)S\(^\circ\) in J K\(-\)1 is ___________. (Nearest integer) [Given : Faraday constant = 96487 C mol\(-\)1]
\(C{d_{(s)}} + H{g_2}S{O_{4(s)}} + {9 \over 5}{H_2}{O_{(l)}}\) \(\rightleftharpoons\) \(CdS{O_4}.{9 \over 5}{H_2}{O_{(s)}} + 2H{g_{(l)}}\)
The value of \(E_{cell}^0\) is 4.315 V at 25\(^\circ\)C. If \(\Delta\)H\(^\circ\) = \(-\)825.2 kJ mol\(-\)1, the standard entropy change \(\Delta\)S\(^\circ\) in J K\(-\)1 is ___________. (Nearest integer) [Given : Faraday constant = 96487 C mol\(-\)1]