`H_(2)(g)+Br_(2)(g) rarr 2HBr(g), DeltaH^(Theta) =-72.40 kJ`
`DeltaG^(Theta) = - 106.49 kJ, T = 298 K`
The value `DeltaS` is ………. .

Calculate the standard free energy change for the reaction: H_(2)(g) +I_(2)(g) rarr 2HI(g), DeltaH^(Theta) = 51.9 kJ mol^(-1) Given: S^(Theta) (H_(2)) = 130.6 J K^(-1) mol^(-1) , S^(Theta) (I_(2)) = 116.7 J K^(-1) mol^(-1) and S^(Theta) (HI) = 206.8 J K^(-1) mol^(-1) .

Calculate the standard free energy change for the reaction: H_(2)(g) +I_(2)(g) rarr 2HI(g), DeltaH^(Theta) = 51.9 kJ mol^(-1) Given: S^(Theta) (H_(2)) = 130.6 J K^(-1) mol^(-1) , S^(Theta) (I_(2)) = 116.7 J K^(-1) mol^(-1) and S^(Theta) (HI) =- 206.8 J K^(-1) mol^(-1) .

The enthalpy changes for two reactions are given by the equations: 2Cr(s) +(3)/(2)O_(2)(g) rarr Cr_(2)O_(3)(s), DeltaH^(Theta) =- 1130 kJ C(s) +(1)/(2)O_(2)(g)rarr CO(g), DeltaH^(Theta) =- 110 kJ What is the enthalpy change in kJ for the following reactions? 3C(s) +Cr_(2)O_(3)(s) rarr 2Cr(s) +3CO(g)

For the reaction, 4C(graphite) +5H_(2)(g) rarr nC_(4)H_(10)(g) , DeltaH^(Theta) =- 124.73 kJ mol^(-1), DeltaS^(Theta) =- 365.8 J K^(-1) mol^(-1) 4C(graphite) +5H_(2)(g) rarr iso-C_(4)H_(10)(g) DeltaH^(Theta) =- 131.6 kJ mol^(-1), DeltaS^(Theta) =- 381.079 J K^(-1) mol^(-1) Indicate whther normal butane can be spontaneously converted to iso-butane or not.

For the reaction, N_(2)(g) +3H_(2)(g) rarr 2NH_(3)(g) DeltaH =- 95.0 kJ and DeltaS = - 19000 J K^(-1) Calculate the temperature in centigrade at which it will attain equilibrium.

For the reaction: 2H_(2)(g) +O_(2)(g) rarr 2H_(2)O(g), DeltaH =- 571 kJ bond enegry of (H-H) = 435 kJ and of (O=O) = 498 kJ . Then, calculate the average bond enegry of (O-H) bond using the above data.

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.

H_(2)O(l) rarr H_(2)O(g), DeltaH = +40.7 kJ DeltaH is the heat of ……………..of water.

H_(2)O(g) rarr H_(2)O(l), DeltaH =- 40.7 kJ DeltaH is the heat of……………….of water.

The standard Gibbs free energies for the reaction at 1773K are given below: C(s) +O_(2)(g) rarr CO_(2)(g), DeltaG^(Theta) =- 380 kJ mol^(-1) 2C(s) +O_(2)(g) hArr 2CO(g),DeltaG^(Theta) =- 500 kJ mol^(-1) Discuss the possibility of reducing Al_(2)O_(3) and PbO with carbon at this temperature, 4Al +3O_(2)(g) rarr 2Al_(2)O_(3)(s),DeltaG^(Theta) =- 22500 kJ mol^(-1) 2Pb +O_(2)(g) rarr 2PbO(s),DeltaG^(Theta) =- 120 kJ mol^(-1)