[" For the reaction at "298K],[qquad [A(g)+B(g)rightleftharpoons C(g)+D(g)],[AH^(@)=-29.8kcal;Delta S^(@)=-0.1kcal/K]],[" Calculate "K.]

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 at 298 K A(g) + B(g) hArr C(g) + D(g) If DeltaH^(@) =29.8 Kcal and DeltaS^(@)=0.1 Kcal K^(-1) then calculate reaction constant (k)

For the reaction at 298 K A(g) + B(g) hArr C(g) + D(g) If DeltaH^(@) =-29.8 Kcal and DeltaS^(@) Kcal K^(-1) then calculate reaction constant (k)

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))hArrD_((g))+C_((g)) DeltaH^(@)=29.8 kcal and DeltaS^(@)=100calK^(-1) . Calculate 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 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 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 : 3A(g)+B(g)to2C(g)+4D(l) Delta U^(@)=50kcal//"mole" and DeltaS^(@)=-400cal//"mol-K". Calculate DeltaG^(@) at 200K:

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).