Thermodynamics ...

∆H = 30 kJ mol^–1, ∆S = 75 J / k / mol. Find boiling temperature at 1 atm.

Spontaneous adsorption of a gas on a solid surface is exothermic process because

There is 1 mol liquid (molar volume 100 ml) in an adiabatic container initial, pressure being 1 bar Now the pressure is steeply increased to 100 bar, and the volume decreased by 1 ml under constant pressure of 100 bar. Calculate ∆H and ∆E. [Given 1 bar = 105 N/m²]

The ratio of P to V at any instant is constant and is equal to 1, for a monoatomic ideal gas under going a process. What is the molar heat capacity of the gas

The entropy values (in J K^–1 mol^–1) of H2 (g) = 130.6 Cl₂(g) = 223 and HCl(g) = 186.7 at 298 K and 1 atm pressure are given. Then entropy change for the reaction.

A mixture of 2 mole of CO(g) and one mole of O₂ in a closed vessel, is ignited to convert the carbon monoxide to carbon dioxide. If ∆H and ∆U are enthalpy and internal energy change. Then

For the reaction of one mole zinc dust with one sulphuric acid in a bomb calorimeter, ∆U and w correspond to :

If the enthalpies of formation of Al₂O₃ and Cr₂O₃ are – 1596 kJ and – 1134 kJ respectively, then the value of ∆H for the reaction ; 2Al + Cr₂O₃ → 2Cr + Al₂O₃ is :

The internal energy change when a system goes from state A to B is 40 kJ/mole. If the system goes from A to B by a reversible path and returns to state A by an irreversible path what would be the net change in internal energy

∆G° for the reaction x + y → z is – 4.606 kcal. The value of equilibrium constant of the reaction at 227°C is : (R = 2.0 cal K^–1 mol^–1 )