∆ {\G}^{\circ} (in {\kJ} {\mol}{ }^{-1} ) for the cell reaction is {\Cu}^{2+}( {\aq})+ {\Fe}( { s}) \to {\Fe}^{2+}( {\aq})+ {\Cu}( { s}) { [ {\Given}_{ {\E}^{\circ}}^{ {\Cu}^{2+} \/ {\Cu}}=0.34 {\V}, {\E}_{ {\Fe}^{2+} \/ {\Fe}}^{\circ}=-0.44 {\V}and {\F}=96,500 {\C} {\mol}^{-1}] {\Cu}^{2+}( {\aq})+ {\Fe}( { s}) \to {\Fe}^{2+}( {\aq})+ {\Cu}( { s})

AP EAMCET 22 May 2023 Shift 2 Paper

Question : 143 of 160

Marks: +1, -0

∆G∘ (in kJ‌mol‌‌−1 ) for the cell reaction is
Cu2+(aq)+Fe( s)→Fe2+(aq)+Cu( s)
[GivenE∘Cu2+∕Cu=0.34V,EFe2+∕Fe∘=−0.44Vand F=96,500Cmol−1]
Cu2+(aq)+Fe( s)→Fe2+(aq)+Cu( s)

+150.5
−150.5
+140.2
−140.2

Validate

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