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 Delta H-DeltaU at 25^@C for the reaction: H_2(g)+( 1/2)O_2(g) = H_2O(l) .

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 DeltaG^(0) for the reaction H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l) at 298K. Given, at 298K DeltaH_(f)^(0) for H_(2)O(l) is -286 kJ *mol^(-1) and the molar entropies (S^(0)) for H_(2)(g),O_(2)(g) and H_(2)O(l) are 130.7, 205.1 and 69.9 J*K^(-1)*mol^(-1) respectively.

Calculate the value of K_c for the given reactions: N_2O_4(g)hArr 2NO_2(g),K_p=11 ( at 100^(@)C )

Assertion DeltaH and DeltaE are almost the same for the reaction, N_2(g) + O_2(g) iff 2NO(g) Reason All reactants and products are gases.

Calculate the value of K_c for the given reactions: SO_2(g)+1/2O_2(g)toSO_3(g) , K_p=2.2 (at 100^(@)C )

Calculate standard enthalpy for the reaction at 298K: C_(2)H_(5)Cl(g)toC_(2)H_(4)(g)+HC l(g) . Given: DeltaH^(0)(C-H)=413kJ*mol^(-1),DeltaH^(0)(C-C)=346kJ*mol^(-1) , DeltaH^(0)(C=C)=611kJ*mol^(-1),DeltaH^(0)(C-Cl)=339kJ*mol^(-1) , DeltaH^(0)(H-Cl)=432kJ*mol^(-1) .

In the reaction N_(2(g)) + O_(2(g)) to 2NO_((g)), DeltaH^@ reaction is + 179.9 kJmol^(-1) and DeltaS_("reaction")^@ = 66.09 JK^(-1)mol^(-1) . Calculate DeltaG^@ reaction at 300K.

DeltaH^@ & DeltaS^@ for the reaction H_2 (g) + I_2 (g) = 2 HI (g) are 16.23 Kj mol^-1 and 63.8 kj mol^-1 predic whether the reaction be spontaneous at 35^@C .

Calculate DeltaH^(0) for the following reaction at 298K: C_(2)H_(2)(g)+CO(g)+H_(2)O(l)toC_(2)H_(3)COOH(l) Given: at 298K temperature, C_(2)H_(3)CO_(2)H(l)+3O_(2)(g)to3CO_(2)(g)+2H_(2)O(l),DeltaH^(0)=-1368kJ 2C_(2)H_(2)(g)+5O_(2)(g) to 4CO_(2)(g)+2H_(2)O(l),DeltaH^(0)=-2600kJ 2CO(g)+O_(2)(g) to 2CO_(2)(g),DeltaH^(0)=-566kJ .