Consider the reaction at 298 K. C(graphite)+2 H 2 (g)⟶ CH 4 (g)Δ?°=−74.6 kJ C(graphite)+2H2(g)⟶CH4(g)ΔH°=−74.6 kJ Calculate the quantities.
Delta Ssys=_______ J/K
Delata Ssurr =_______ J/K
Given that
C (graphite) + 2H2(g) ---> CH4(g) Δ?° = −74.6 kJ = -74600 J
Ssys = So(products) - So(reactants) = So(CH4) - So(graphite) - (2*So(H2))
From Literature,
So(CH4) = 186.25 J/K.mol
So(graphite) = 5.74 J/K.mol
So(H2) = 130.68 J/K.mol
(a) Ssys = (186.25 J/K.mol) - (5.74 J/K.mol + (2* 130.68 J/K.mol)) = -80.8 J/K.mol
(b) Ssurr = -H/T = 74600 J / 298 K = 250.3 J/K
Consider the reaction at 298 K. C(graphite)+2 H 2 (g)⟶ CH 4 (g)Δ?°=−74.6 kJ C(graphite)+2H2(g)⟶CH4(g)ΔH°=−74.6 kJ...
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