In the given reaction, calculate the standard free energy change at `25^(@)C:N_(2)(g)+3H_(2)(g)to2NH_(3)` [Given that, `DeltaH^(0)=-91.8kJ and DeltaS^(0)=-198J*K^(-1)`]

Calculate the standard free energy change for the reaction, N_(2(g))+3H_(2(g))to2NH_(3(g)) at 298 K . Given, DeltaH^@ =-92.4kJ and DeltaS^@ = -198.3 JK^(-1) . Also, comment on the result.

Determine standard free energy DeltaG^@" at " 25^@C for the reaction N_2(g) + 3H_2(g) hArr 2NH_3(g) Given: DeltaH^@ = -91.8 kJ , DeltaS^@ = - 198 J K^(-1)

Calculate the standard free energy change for the reaction : H_(2)(g) + I_(2)(g) to 2HI(g) DeltaH^(@) = 51.9 kJ "mol"^(-1) Given : S^(@)(H_(2)) = 130.6 J K^(-1) "mol"^(-1) S^(@)(I_(2)) = 116.7 J K^(-1) "mol"^(-1) and S^(@)(HI) = 206.3 J K^(-1) "mol"^(-1) .

Calculate the DeltaG^0 for the reaction N_2(g) + O_2(g) * 2NO(g) Given DeltaH^0 =180.5 K.J , and DeltaS^0 = 15 J at 25^@C .

Calculate the free eneryg change at 298 K for the reaction , Br_(2)(l)+Cl_(2)(g) to BrCl(g) . For the reaction DeltaH^(@)=29.3 kJ &

The equilibrium constant for the reaction given below is 2.0xx10^(-7) at 300K. Calculate the standard free energy change for the reaction, PCl_(5(g))hArrPCl_(3(g))+Cl_(2(g)) . Also, calculate the standard entropy change if DeltaH^@=28.40kJmol^(-1) .

Calculate the standard free energy change Delta G^(@) for the reaction, 2HgO(s) rarr 2Hg(l) + O_(2)(g) Delta H^(@) = 91 kJ mol^(-1) at 298 K, S_((HgO))^(@) = 72.0 JK^(-1) mol^(-1) .