For the reaction
`2A(g)+B(g)rarr2D(g)`
`DeltaU^(theta)=-10.55 KJ and Delta S^(theta)=-44.1 JK^(-1)`
Calculate `DeltaG^(Ө)` for the reaction, and predict whether the reaction may occur spontaneously

For the reaction, 2A(g)+B(g) rarr 2D(g) DeltaU^(Θ)=-10.5 kJ and DeltaS^(Θ)=-44.1 JK^(-1) Calculate DeltaG^(Θ) for the reaction, and predict whether the reaction may occur spontaneously.

For reaction, 2K_((g))+L_((g))rarr2M_((g)),DeltaU^(@)=-"10.5 KJ and "DeltaS^(@)=-"44.1 J K"^(-1) . Calculate DeltaG^(@) for the reaction and predict whether the reaction will be spontaneous or non-spontaneous?

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).

For the reaction, A(s) + 3B(g) rarr 4C(g) + d(l) Delta H and Delta U are related as :

Predict whether it is possible or not to reduce magnesium oxide using carbon at 298K according to the reaction. MgO(s) +C(s) rarr Mg(s) +CO(g) Delta_(r)H^(Theta) = +491.18 kJ mol^(-1) and Delta_(r)S^(Theta) = 197.67 J K^(-1) mol^(-1) If not at what temperature, the reaction becomes spontaneous.

For the reaction, N_(2)(g) +3H_(2)(g) rarr 2NH_(3)(g) DeltaH =- 95.0 kJ and DeltaS = - 19000 J K^(-1) Calculate the temperature in centigrade at which it will attain equilibrium.

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

If for a reaction A(s) rarr 2B(g), deltaU+ 1.2 kcal and deltaS=40 cal K^(-1) at 400K then deltaG for the reaction will be ( R=2 cal mol^(-1)K^(-1)

For a hypothetical reaction A(g) + 3B(g) to 2C(g). Delta H = -100 kJ and Delta S = -200 Jk^(-1) . Then the temperature at which the reaction will be in equilibrium is

For the reaction N_(2)(g) + 3H_(2) rarr 2NH_(3)(g) Delta H = - 95.4 kJ and Delta S = -198.3 JK^(-1) Calculate the temperature at which Gibbs energy change (Delta G) is equal to zero. Predict the nature of the reaction at this temperature and above it.