Consider the following reaction at 298 K. C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K...

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Consider the following reaction at 298 K. C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K...

Consider the following reaction at 298 K.

C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K

Calculate the following quantities.

ΔSsys=ΔSsys

J/K

ΔSsurr=

J/K

ΔSuniv=

J/K

science chemistry

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Answer 1

Answer #1

C(graphite) + 2H2(g)⟶CH4(g) ΔHo = −74.6 kJ and ΔSo= −80.8 J/K

ΔSsys = ΔSo

ΔSsys = − 80.8 J/K

n surt Assurr =

ΔHosurr = − ΔHo

ΔHosurr = 74.6 kJ

ΔSsurr = 250.3 J/K

ΔSuniv = ΔSsys + ΔSsurr

ΔSuniv = − 80.8 J/K + 250.3 J/K

ΔSuniv = 169.5 J/K

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Answer 2

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Consider the following reaction at 298 K. C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K...

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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...