[" For the equilition "2H_(2)(g)+O_(2)(g)rightleftharpoons2H_(2)O(d)at25^(@)C,AG^(n)" is "-474.78ldmol^(-1)" .Calculate "log" ? "],[" for it "R=8.314JK^(-1)mol^(-1)" )."]

For the equilibrium reaction: 2H_(2)(g) +O_(2)(g) hArr 2H_(2)O(l) at 298 K DeltaG^(Theta) = - 474.78 kJ mol^(-1) . Calculate log K for it. (R = 8.314 J K^(-1)mol^(-1)) .

For the equilibrium reaction: 2H_(2)(g) +O_(2)(g) hArr 2H_(2)O(l) at 298 K DeltaG^(Theta) = - 474.78 kJ mol^(-1) . Calculate log K for it. (R = 8.314 J K^(-1)mol^(-1)) .

K_(c)" for "CS_(2)(g)+4H_(2)(g)hArrCH_(4)(g)+2H_(2)S(g) is 0.28 at 900K. Calculate K_(p) . (R = 8.314 JK^(-1)mol^(-1) ).

Calculated the equilibrium constant for the following reaction at 298K : 2H_(2)O(l) rarr 2H_(2)(g) +O_(2)(g) Delta_(f)G^(Theta) (H_(2)O) =- 237.2 kJ mol^(-1),R = 8.314 J mol^(-1) K^(-1)

Calculated the equilibrium constant for the following reaction at 298K : 2H_(2)O(l) rarr 2H_(2)(g) +O_(2)(g) Delta_(f)G^(Theta) (H_(2)O) =- 237.2 kJ mol^(-1),R = 8.314 J mol^(-1) K^(-1)

Calculate the Delta H at 298 K for the reaction (1)/(2)N_(2)(g) + (3)/(2)H_(2)(g) rarr NH_(3)(g) given that Delta H for the formation of NH_(3) has a valve of -46.0 kJ mol^(-1) (R = 8.314 JK^(-1) mol^(-1)) .

Calculate DeltaH for the reaction H_(2)(g)+1//2O_(2)(g)toH_(2)O(g) given the bond energies of H-H and O=O bonds and O-H bond are 433 kJ mol^(-1) , 492 kJ mol^(-1) and 464kJ" "mol^(-1) .