For the reaction at 300 K
`A(g)+B(g)toC(g)" Delta"E=-3.0"kcal",DeltaS=-10.0cal//K` value of `DeltaG` is

For the f reaction at 300K A(g)+B(g) to C(g) DeltaU = - 3.0 k cal" "," "DeltaS = - 10.0 cal //K Value of the DeltaG is

For the reaction at 288 K A(g)+B(g) iff C(g) +D(g) , DeltaH^@ = - 29.8kcal and DeltaS^@ =- 100cal_/K . Find the value of equilibrium constant.

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 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.

For the reaction at 298 K A(g) + B(g) iff C(g)+ D(g) DeltaH^(@) = -29.8 Kcal, DeltaS^(@) = - 0.1 Kcal //K Calculate DeltaG^(@) and K.

For the reaction 2A (g) + B(g) to C (g) Delta U^(@) = 20 kcal/mole, Delta S^(@) = 100 cal/kmole at 300 K. Hence Delta G^(@) in kcal is __________ [R = 2 cal mol^(-1) K^(-1)]

For the reaction 2A (g) + B(g) to C (g) Delta U^(@) = 20 kcal/mole, Delta S^(@) = 100 cal/kmole at 300 K. Hence Delta G^(@) in kcal is __________ [R = 2 cal mol^(-1) K^(-1)]

For the reaction, X_(2)O_(4)(l)rarr2XO_(2)(g) , DeltaE=3.1Kcal , DeltaS=30cal//K at 300K . Hence DeltaG is

For the reaction, X_(2)O_(4)(l)rarr2XO_(2)(g),DeltaE=2.1Kcal , DeltaS=20cal//K at 300K . Hence DeltaG is