The equilibrium constant for the reaction {\M}( { s})+2 {\Ag}^{+}( {\aq}) \rightarrow {\M}^{2+}( {\aq})+2 {\Ag}( { s}) is 10^{15}. What is the Gibbs energy change ( ∆_r G^{⊖} in {\KJ} {\mol}^{-1} ) for this reaction? ( { {\RT}}/{ {\F}} \times 2.303=0.06 {\V} ; {\F}=96500 {\C} {\mol}^{-1}) .

TG EAMCET 30 Apr 2025 Shift 1 Paper

Question : 143 of 160

Marks: +1, -0

The equilibrium constant for the reaction M( s)+2Ag+(aq)⟶M2+(aq)+2‌Ag( s) is 1015. What is the Gibbs energy change ( ∆rG⊖ in KJ‌mol−1 ) for this reaction?
(‌

×2.303=0.06V;F=96500Cmol−1).

‌−86850
‌−96500
‌−86.85
‌−96.5

Validate

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