For the reaction
2A+ B ---> 2D
delta U = - 10.5 KJ and delta S= - 44.1 JK-1mol-1
Calculate delta G for the reaction and predict whether the reaction may occur spontaneously ( R = 8.314 J K-1 mol-1 )
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For the given reaction,
2 A ( g ) + B ( g ) → 2D ( g )
Δ n g = 2 – (3)
= –1 mole
Substituting the value of Δ U θ in the expression of Δ H :
Δ H θ = Δ U θ + Δ n g R T
= (–10.5 kJ) – (–1) (8.314 × 10 –3 kJ K –1 mol –1 ) (298 K)
= –10.5 kJ – 2.48 kJ
Δ H θ = –12.98 kJ
Substituting the values of Δ H θ and Δ S θ in the expression of Δ G θ :
Δ G θ = Δ H θ – T Δ S θ
= –12.98 kJ – (298 K) (–44.1 J K –1 )
= –12.98 kJ + 13.14 kJ
Δ G θ = + 0.16 kJ
2 A ( g ) + B ( g ) → 2D ( g )
Δ n g = 2 – (3)
= –1 mole
Substituting the value of Δ U θ in the expression of Δ H :
Δ H θ = Δ U θ + Δ n g R T
= (–10.5 kJ) – (–1) (8.314 × 10 –3 kJ K –1 mol –1 ) (298 K)
= –10.5 kJ – 2.48 kJ
Δ H θ = –12.98 kJ
Substituting the values of Δ H θ and Δ S θ in the expression of Δ G θ :
Δ G θ = Δ H θ – T Δ S θ
= –12.98 kJ – (298 K) (–44.1 J K –1 )
= –12.98 kJ + 13.14 kJ
Δ G θ = + 0.16 kJ
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