Given that:
`DeltaG_(F)^(@)(CuO) =-30.4 "Kcal"//"mole"`
`DeltaG_(f)^(@)(Cu_(2)O)=-34.98 Kcal//"mole" " "T=298K`
Now on the basis of above data which of the following predications will be most appropriate under the standard conditons and reversible reaction.

For reaction at 1000k : A(g)Leftrightarrow B(g),DeltaG_(f)^(@)(A,g)=-5.2 kcal//"mole"^(-1) , DeltaG_(f)^(@)(B,g)=-3.814 kcal//"mole"^(-1) Equillibrium constant of reaction is:

For the reaction: N_(2)O_(4)(g) hArr 2NO_(2)(g) (i)" " In a mixture of 5 mol NO_(2) and 5 mol N_(2)O_(4) and pressure of 20 bar. Calculate the value of DeltaG for the reaction. Given DeltaG_(f)^(@) (NO_(2)) = 50 KJ/mol, DeltaG_(f)^(@) ((N_(2)O_(4)) =100 KJ/mol and T=298 K. (ii) Predict the direction in which the reaction will shift, in order to attain equilibrium [Given at T=298 K, 2.303 "RT" = 5.7 KJ/mol.]

For the reaction: N_(2)O_(4)(g) hArr 2NO_(2)(g) (i)" " In a mixture of 5 mol NO_(2) and 5 mol N_(2)O_(4) and pressure of 20 bar. Calculate the value of DeltaG for the reaction. Given DeltaG_(f)^(@) (NO_(2)) = 50 KJ/mol, DeltaG_(f)^(@) ((N_(2)O_(4)) =100 KJ/mol and T=298 K. (ii) Predict the direction in which the reaction will shift, in order to attain equilibrium [Given at T=298 K, 2.303 "RT" = 5.7 KJ/mol.]

For the reaction: N_(2)O_(4)(g) hArr 2NO_(2)(g) (i)" " In a mixture of 5 mol NO_(2) and 5 mol N_(2)O_(4) and pressure of 20 bar. Calculate the value of DeltaG for the reaction. Given DeltaG_(f)^(@) (NO_(2)) = 50 KJ/mol, DeltaG_(f)^(@) ((N_(2)O_(4)) =100 KJ/mol and T=298 K. (ii) Predict the direction in which the reaction will shift, in order to attain equilibrium [Given at T=298 K, 2.303 "RT" = 5.7 KJ/mol.]

While analyzing driving forces for a chemical reaction it is observed that energy and entropy are true forces. The entropy is a typical state function owing to the possibility of calculation of its absolute value. The absolute values of entropies can be compared an calculating by knowing the residual entropies at 0 K and by calculating the change due to change of state. Using the given information and data for a particular substance x answer the questions that follow : Useful data : (p) Standard melting point and boiling point of x is 200 K and 400 K respectively. (q) DeltaH_("fusion")^(@) = 10 kcal//"mole" and DeltaH_(vap)^(@) = 80 kcal//"mole" . (r) C_(p.m)(s) x = 0.1T cal//K "mole" , C_(p.m) (l) x = 0.05 Tcal//K "mole S_(m.40 K)^(@)s_(x) = 5 cal//"mole" Which of the following options regarding absolute molar entropies of x is/are correct?

(a) In the following equilibrium N_(2)O_(4)(g)hArr2NO_(2)(g) when 5 moles of each are taken, the temperature is kept at 298K the total pressure was found to be 20 bar. Given that DeltaG_(f)^(@)(N_(2)O_(4))=100kJ, DeltaG_(f)^(@)(NO_(2))=50kJ (i) Find DeltaG of the reaction. (ii) The direction of th reaction in which the equilibrium shifts. (b) A graph is plotted for a real gas which follows van der Waals' equation with pV_(m) taken on Y -axis and p on X -axis. Find the intercept of the ine where V_(m) is molar volume.

While analyzing driving forces for a chemical reaction it is observed that energy and entropy are true forces. The entropy is a typical state function owing to the possibility of calculation of its absolute value. The absolute values of entropies can be compared an calculating by knowing the residual entropies at 0 K and by calculating the change due to change of state. Using the given information and data for a particular substance x answer the questions that follow : Useful data : (p) Standard melting point and boiling point of x is 200 K and 400 K respectively. (q) DeltaH_("fusion")^(@) = 10 kcal//"mole" and DeltaH_(vap)^(@) = 80 kcal//"mole" . (r) C_(p.m)(s) x = 0.1T cal//K "mole" , C_(p.m) (l) x = 0.05 Tcal//K "mole S_(m.40 K)^(@)s_(x) = 5 cal//"mole" Which of the following statement is/are true ?