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Given :Ag+2Bg→ Cg ΔrCP=0ΔfH°(C,g)=-200 kJ mol-1,ΔfH°(B,g)=-20 kJ mol-1,ΔfH°(A,g)=-120 kJ mol-1Sm°(C,g)=250 J mol-1 K-1, Sm°(B,g)=30 J mol-1 K-1, Sm°(A,g)=200 J mol-1 K-1All data at 400 K temperature. Which is/are correct statement(s)?

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a

Change in entropy of reaction at 400 K is −10 JK−1

b

Change in enthalpy of reaction at 400 K is -40 kJ

c

Change in entropy of surrounding at 400 K is 100 JK−1

d

Change in free energy of reaction is 35 kJ at 500 K

answer is A.

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Detailed Solution

1) ΔS°=SCo−SAo−2SBo=250−200−230=−10 JK−1 mol−12) ΔH°=ΔFH°C−ΔFH°A−2ΔFH°B=200−−120−2−20=-403) ΔSsurro=qsurrT=−qsysT=+40×1000400=+1004) ΔG°=ΔH°−TΔS°=−40−500−101000=−40+5=-35

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Given :Ag+2Bg→ Cg ΔrCP=0ΔfH°(C,g)=-200 kJ mol-1,ΔfH°(B,g)=-20 kJ mol-1,ΔfH°(A,g)=-120 kJ mol-1Sm°(C,g)=250 J mol-1 K-1, Sm°(B,g)=30 J mol-1 K-1, Sm°(A,g)=200 J mol-1 K-1All data at 400 K temperature. Which is/are correct statement(s)?