41% Hi Decomposes into `H_2` and `I_2` at 300K calculate delta g ?

For the reaction , H_(2)(g) + I_(2) (g) hArr 2HI(g), K = 55.3 " at " 699 K. In a mixture consisting of 0.70 atm of HI and 0.02 atm each of H_(2) and I_(2) at 699 K, will there be any net reaction ? If so will HI be consumed or formed ?

For the reaction: CO(g) +H_(2)O(g) hArr CO_(2)(g) +H_(2)(g) (Delta_(r)H)_(300K) = 41.2 kJ mol^(-1) (Delta_(r)H)_(1200K) =- 33.0 kJ mol^(-1) (Delta_(r)S)_(300K) = -4.2 xx 10^(-2) kJ mol^(-1) (Delta_(r)S)_(1200K) =- 3.0 xx10^(-2) kJ mol^(-1) Predict the direction of spontaneity of the reaction at 300K and 1200K . also calculated log_(10)K_(p) at 300K and 1200K .

For a reversible process at T = 300K, the volume is increased from V_(i)=1L to V_(f)=10L . Calculate Delta H if the process is isothermal -

When 2.00 mol each of H_2(g) and I_2(g) are reacted in a 1.00 L container at a certain temperature , 3.50 mol of HI is present at equilibrium.Calculate the value of the equilibrium constant , K_c for the reaction : H_2+I_2hArr 2HI

The value of K_(c) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) is 64 at 773K . If one "mole" of H_(2) , one mole of I_(2) , and three moles of HI are taken in a 1 L flask, find the concentrations of I_(2) and HI at equilibrium at 773 K .

If for the reaction [2A(I) rarr 4B(g)] delta U and deltaS respectively are 1.2 kcal and 10 cal K^-1 at 300 K then delta G for the reaction is