1. ⇒ (MHT CET 2023 12th May Morning Shift )
Calculate Δ G ∘ for the reaction Mg ( s ) + Sn ( aq ) + + ⟶ Mg ( aq ) + + + Sn ( s ) if E cell 0 is 2.23 V .
A. − 430.4 kJ
B. 215.2 kJ
C. 645.6 kJ
D. − 860.8 kJ
Correct Option is (A)
Δ G ∘ = − nFE cell ∘ = − 2 × 96500 × 2.23 = − 430390 J = − 430.4 kJ
2. ⇒ (MHT CET 2023 9th May Morning Shift )
Calculate Δ G ∘ for the cell:
Sn ( s ) | Sn ( 1 M ) + | | Ag ( 1 M ) + | Ag ( s ) at 25 ∘ C ( E cell ∘ = 0.90 V )
A. − 173.7 kJ
B. − 225.3 kJ
C. − 100.2 kJ
D. − 290.8 kJ
Δ G ∘ = − nF E cell ∘ = − 2 × 96500 × 0.90 = − 173700 J = − 173.7 kJ