For reaction at `1000k`:
`A(g)Leftrightarrow B(g),DeltaG_(f)^(@)(A,g)=-5.2 kcal//"mole"^(-1)`,
`DeltaG_(f)^(@)(B,g)=-3.814 kcal//"mole"^(-1)`
Equillibrium constant of reaction is:

For a reaction: 2A(g)+B(g)toC(g), DeltaU^(@)=30kcal//"mole" , DeltaS^(@)=100cal//K"mole". "What will be the value of" DeltaG_(reaction)^(@)at 400K? [R=2cal//K"mole"]" "[DeltaC_(p_(reaction))=0]

For a reaction : 3A(g)+B(g)to2C(g)+4D(l) Delta U^(@)=50kcal//"mole" and DeltaS^(@)=-400cal//"mol-K". Calculate DeltaG^(@) at 200K:

For a reaction: 2A(g)+4B(g)to 5C(g)+2D(l)DeltaE^(@)=40kca\l//"mole" and DeltaS^(@)=+200cal//K"mole" The value of DeltaG_(200)^(@) will be.

Given that: DeltaG_(F)^(@)(CuO) =-30.4 "Kcal"//"mole" DeltaG_(f)^(@)(Cu_(2)O)=-34.98 Kcal//"mole" " "T=298K Now on the basis of above data which of the following predications will be most appropriate under the standard conditons and reversible reaction.

Given that: DeltaG_(F)^(@)(CuO) =-30.4 "Kcal"//"mole" DeltaG_(f)^(@)(Cu_(2)O)=-34.98 Kcal//"mole" " "T=298K Now on the basis of above data which of the following predications will be most appropriate under the standard conditons and reversible reaction.

For the reaction at 298 k, A(g) +B(g) hArr C(g) +D(g) DeltaH_0=-29.8 kcal, DeltaS^@=-0.100 kcal K^(-1) Find the value of equilibrium constant at the same temp.