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.

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)+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 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 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 298K: A_((g)) +B_((g)) hArr C_((g)) + D_((g)) Delta H^(@) + 29.8kcal and Delta S^(@) = 100cal K^(-1) . Find the value of equilibrium constant.

For the reaction at 298K: A_((g)) +B_((g)) hArr C_((g)) + D_((g)) Delta H^(@) + 29.8kcal and Delta S^(@) = 100cal K^(-1) . Find the value of equilibrium constant.

For the reaction, 2A (s) + 2B (g)to C (g) + D(s) at 298K Delta U ^(@) =-10.5KJ and Delta S ^(@)=-44.10 JK^(-1) Calculate Delta G ^(@) for the reaction (in Joules).