Theoretical basics of Inorganic chemistry

1.      At 25°C (298 K), the reduction of copper(I) oxide is nonspontaneous ∆G = 8.9 kJ). Calculate the temperature at which the reaction becomes spontaneous.

2.      Determine ∆_rGº at 298.15 K for the reaction 4Fe(s) + 3O₂(g) → 2Fe₂O₃(s). ∆_rHº = -1648 kJ mol^-1 and ∆_rSº = -549.3 Jmol^-1K^-1.

3.      For the reaction below, ∆_rGº = 326.4 kJ mol^-1 , 3O₂(g) → 2O₃(g). What is the Gibbs energy change for the system when at 1 bar reacts completely to give O₃(g) at 1 bar?

4.      What is the minimum value of Q required to make the reverse reaction, conversion of NH₃ to N₂ and H₂, spontaneous at 298 K?

5.      What is the partial pressure of NH₃ in the ammonia synthesis reaction if the Gibbs energy of reaction is –82.00 kJ mol–1 and the partial pressures of hydrogen and nitrogen are each 0.500 bar? The temperature is 298 K.

6.      The reaction of 1.0 mol of C to form carbon monoxide in the reaction 2C(s) + O₂ (g) → 2CO(g) releases 113 kJ of heat. How much heat will be released by the combustion of 100 g of C according the above information?

7.      Use bond energies to estimate the enthalpy change for: N₂(g) + 3H₂(g) → 2NH₃(g)  Compare the value you obtained using average bond energies to that which you would obtain using standard heats of formation.

8.      Calculate ∆Hº for the reaction: GeO(s) + ½ O₂(g) → GeO₂(s) by combining the enthalpies of these two known equations, using Hess’ss Law.

Ge(s) + ½O₂(g) → GeO(s) ∆Hº = -255 kJ

GeO₂(s) → Ge(s) + O₂(g) ∆Hº = +535 kJ

9.      From the following enthalpy changes,

Cu(s) + Cl₂(g) → CuCl₂(s) ∆H° = -206 kJ

2Cu(s) + Cl₂(g) → 2CuCl(s) ∆H° = -136 kJ

calculate the value of ∆H° for the reaction CuCl₂(s) + Cu(s) → 2CuCl(s).

10.  How much heat, in kilojoules (kJ), is required to raise the temperature of 237 g of cold water from 4.0 to 37.0ºC (body temperature)?