For the reaction, `2A rarr A_2` following data is obtained at 298K. `triangleU = -20KJ`, `triangleS= -30J` then find `triangle G`

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).

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

For the reaction, 2NOCl(g) hArr 2NO(g)+Cl_(2)(g) Calculate the standard equilibrium constant at 298 K . Given that the value of DeltaH^(ɵ) and DeltaS^(ɵ) of the reaction at 298 K are 77.2 kJ mol^(-1) and 122 J K^(-1) mol^(-1) .

For a demerization reaction , 2A (g) to A_2 (g) at 298 K, Delta U(Theta) = - 20 kJ"mol"^(-1), Delta S^(Theta) = - 30 JK^(-1) "mol"^(-1) , then the Delta G^(Theta) will be _________J.

For the reaction at 298K ; [A_(2)B_(4)rightarrow2AB_(2)] , Delta H=2kJ and Delta S=20J/K at , constant P and T " ,the reaction will be ("A") Spontaneous and entropy driven " "(B)" spontaneous and enthalpy driven " "(C)" Non- spontaneous " "(D)" at equilibrium "

The value of Delta H for the reaction 2 N_(2)(g) + O_(2) (g) rarr 2N_(2) O (g) at 298 K is 164 kJ . Calculate Delta U for the reaction. Strategy : In this process, 3 mol of gas change to 2 mol of gas at constant temperature and pressure. Assuming ideal gas behavior, we can use. First Delta_(n_(g)) and the obtain a value of Delta U by converting the value of Delta H from 164 kJ to 164000 J and expressing R in units of J mol^(-1) K^(-1)

For the reaction CO (g) + (1)/(2) O_(2) (g) rarr CO_(2) (g) Delta H and Delta S are 283 kJ and -87 J K^(-1) , respectively. It was intended to carry out this reaction at 1000,1500,3000, and 3500 K. At which of these temperatures would this reaction be thermodynamically spontaneous?