The chemical equation for conversion of oxygen to Ozone is 3/2O₂ → O₃. We have equation, ΔG = ? 2.303 RT log Kp. So by substituting we get ΔG = ? 2.303 x 8.314 J/K-mol x 293K x 2.47 x 10^-29 = 163000 J/mol = 163 kJ/mol.

The first law of rmodynamics is commonly stated as law of conservation of energy that is energy can neir be created nor be destroyed, in or terms we can also say that energy of an isolated system is constant.

Given that C₂H₆(g) + 3 1/2 O_2(g) → 2CO_2(g) + 3H₂O_(l) As we know that, ΔHr = ? ΔH_f[products] – ? ΔH_f[reactants]; ΔH_c(C₂H₆) = 2 X (-393.5 kJ mol^-1) + 3 X (-285.8 kJ mol^-1) ? (- 84.7 kJ mol^-1) ? 2 X (0 kJ mol^-1) = ΔH_c(C₂H₆) = – 1559.7 kJ mol^-1.

When a work is done or by system, heat passes into out of system and matter enters or leaves system, re is a change in internal energy of system. It is represented by symbol ?U?.

An indirect method, in which we can construct an enthalpy diagram is called a Born-Haber cycle as it is nearly impossible to determine lattice enthalpies directly by experiment. It is an approach to analyze reaction energies.

An intensive property does not depend on quantity or size of object, whereas extensive property depends on quantity and size of object. Here volume, enthalpy and internal energy are extensive properties, while colour is an intensive property.

The enthalpy change that occurs when one mole of a molecule breaks into its atoms is known as enthalpy of atomization. The energy released during conversion of a hydrogen molecule into two hydrogen atoms is enthalpy of atomization.

An open system allows only energy transfer whereas an isolated system neir allows energy nor mass transfer through system from surroundings. Isolated and closed systems are not same. So above statement is false.

According to Helmholtz equation; G = H -TS, when enthalpy H is positive and entropy S is negative, Gibbs free energy is always positive and reaction is not spontaneous at all temperatures.

Using equation ΔG = ΔH – TΔS, where G is represented by Gibbs free energy, H is represented by change in enthalpy, T is represented by temperature and S is represented by entropy. ΔH = ΔG + TΔS = 3.4 kcal – 293 x 2.4 cal/K = 3.4 kcal.