For the reaction at 300K (take `R=8JK^-1mole^-1` `2A(g)+B(s)rarr2D(g)`,`Delta U^(0)=-10kJ` and `Delta S^(0)=-50JK^-1`. Find the value of `Delta G^(0)`

For the reation at 300 K A(g)hArrV(g)+S(g) Delta_(r)H^(@)=-kJ//mol, Delta_(r)S^(@)=-0.1K^(-1).mol^(-1) What is 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).

For the reaction at 300K A(g) hArr V(g)+S(g) Delta_(r) H^(@)=-30kJ //mol , Delta_(r)S^(@)=-0.1Kj.k^(-1).mol^(-1) What is the value of equilibrium constant ?

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 300 K A(g)+B(g)toC(g)" Delta"E=-3.0"kcal",DeltaS=-10.0cal//K value of DeltaG is

For the reaction between CO_(2) and graphite: CO_(2)(g)+C(s)to2CO(g), Delta=170kJ and DeltaS=170.JK^(-1). "The reaction will be spontaneous at":

For the reaction between CO_2 and graphite CO_2(g)+C(s) hArr2CO(g) DeltaH=+170.0kJ and DeltaS = 170 JK^(-1) . The reaction is spontaneous at