Consider the following cell reaction: C d (s) + H g₂ S O 4(s) + 9/5H₂O (l) CdS O₄.9/5H₂O (s) + 2H g (l) The value of E cell ⁰ is 4.315 V at 25° C. If Δ H° = - 825.2 kJ mol⁻¹, the standard entropy change Δ S° in J K⁻¹ is _ _ _ _ _ _. (Nearest integer) [Given: Faraday constant = 96487 C mol⁻¹]

Redox Reactions and Electrochemistry: JEE Main 2021 Chemistry question

JEE Main 2021 · 31 Aug, Morning shift · Q10

JEE Main 202131 Aug, Morning shiftChemistryHardRedox Reactions and Electrochemistry138× since 2002

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

^\circ

-

825.2 kJ mol^

-

1, the standard entropy change

\Delta

^\circ

in J K^

-

1 is ___________. (Nearest integer) [Given : Faraday constant = 96487 C mol^

-

Your answerType your answer. Integers and decimals are accepted.

JEE Main 2021 Redox Reactions and Electrochemistry Question with Answer (31 Aug Morning shift, Q10) | JEE Arc