1. ⇒ (MHT CET 2023 9th May Morning Shift )
Calculate the value of Δ G for following reaction at 300 K .
H 2 O ( s ) ⟶ H 2 O ( l ) ( Δ H = 7 kJ , Δ S = 24.8 J K − 1 )
A. 0.74 kJ mol − 1
B. − 0.82 kJ mol − 1
C. 0.21 kJ mol − 1
D. − 0.44 kJ mol − 1
Correct Option is (D)
Δ H = 7 kJ Δ S = 24.8 J K − 1 = 24.8 × 10 − 3 kJ K − 1 T = 300 K Δ G = Δ H − T Δ S ∴ Δ G = 7 kJ − ( 300 K × 24.8 × 10 − 3 kJ K − 1 ) = 7 kJ − 7.44 kJ = − 0.44 kJ