Define the following terms
(a) isothermal process (b) adiabatic process
(c) isobaric process (d) isochoric process

What are state and path functions? Give two examples

The equilibrium constant of a reaction is 10, what will be the sign of ΔG? Will this reaction be spontaneous?

Define the following terms.

Predict the change in internal energy for an isolated system at constant volume.

One mole of a gaseous system absorbs 100 J of heat and does work equivalent to 50 J. Calculate the change in the internal energy of the system.

Bring out the differences between extensive and intensive properties.

Identify processes under the following conditions
(i) dT = 0
(ii) dP = 0
(iii) dV = 0

Define Standard Entropy.

What is the nature of the reaction for the following?
(i) ΔG>0
(ii) ΔG<0
(iii) ΔG=0

5 moles of an ideal gas expand isothermally and reversibly from a pressure of 10 atm to 2 atm at 300K. Calculate the work done by the system.

Enthalpies of formation of CO(g),CO₂(g), N₂O(g) and N₂O₄(g) are -110, -393, + 81 and + 9.7 kJ mol respectively. Find the value of \(\Delta\)H for the reaction. N₂O₄(g) + 3CO(g) \(\rightarrow\) N₂O(g) + 3CO₂(g).

Urea on hydrolysis produces ammonia and carbon dioxide. The standard entropies of urea, H₂O, CO₂, NH₃ are 173.8, 70, 213.5 and 192.5 J mole^-1K^-1 respectively. Calculate the entropy change for this reaction.

A gas contained in a cylinder fitted with a frictionless piston expands against a constant external pressure of 1 atm from a volume of 5 litres to a volume of 10 litres. In doing so it absorbs 400 J of thermal energy from its surroundings. Determine the change in internal energy of system.

The standard enthalpies of formation of \(C_2 H_5 OH_{I}, CO_{2{g}}\) and \(H_2 O(_{I})\) are -277, -393.5 and -285.5 kJ mol^-1 respectively. Calculate the standard enthalpy change for the reaction \(C_2O_5 OH_{(I)}+3O_{2{g}} \rightarrow 2CO_{2{g}}+3 H_2 O_{(I)}\). The enthalpy of formation of O_2(g) in the standard state is zero, by definition.

Calculate the value of \(\Delta\)U and \(\Delta\)H on heating 128 g of oxygen from O°C to 100°C. C_v and C_p on an average are 21 and 29 J mol^-1 K^-1. (The difference is 8 J mol^-1 K^-1 which is approximately equal to R)

The enthalpy of formation of methane at constant pressure and 300 K is - 78.84 k.l, What will be the enthalpy of formation at constant volume?

(a) Under what condition, the heat evolved or absorbed in a reaction is equal to its free energy change?
(b) Calculate the entropy change for the following reversible process.
\(H_2 O \rightleftharpoons H_2O_{I} \) Δ_fus H is 6 kJ mol^-1

Prove that for an ideal gas, C_p is greater than C_v.

Calculate \(\triangle_r{G}^{\ominus}\) for conversion of oxygen to ozone, \({3\over 2}{O}_{{2}_{(g)}}\rightarrow{O}_{{3}_{(g)}}\) at 298 K. If Kp for this conversion is 2.47 X 10^-29.

The value of K_c for the following reaction at 717 K is 48.

The value of Kc for the reaction
N₂O₂(g) \(\rightleftharpoons \) 2NO₂(g)

One mole of H₂ and one mole of I₂ are allowed to attain equilibrium in 1 lit container. If the equilibrium mixture contains 0.4 mole of HI. Calculate the equilibrium constant.

The equilibrium concentrations of NH₃, N₂ and H₂ are 1.8 x 10^-2 M, 1.2 x 10^-2 M and 3 x 10^-2 M respectively. Calculate the equilibrium constant for the formation of NH₃ from N₂ and H₂. [Hint: M= mol lit^-1]

The equilibrium constant at 298 K for a reaction is 100.
A + B \(\rightleftharpoons \) C + D
If the initial concentration of all the four species is 1 M, the equilibrium concentration of D (in mol lit^-1) will be

For an equilibrium reaction K_p = 0.0260 at 25° C ΔH= 32.4 kJmol^-1, calculate Kp at 37° C

For the reaction,
A₂(g) + B₂(g) ⇌ 2AB(g) ; ΔH is –ve.
the following molecular scenes represent different reaction mixture (A – green, B – blue)

i) Calculate the equilibrium constant K_P and (K_C).
ii) For the reaction mixture represented by scene (x), (y) the reaction proceed in which directions?
iii) What is the effect of increase in pressure for the mixture at equilibrium.

One mole of PCl₅ is heated in one litre closed container. If 0.6 mole of chlorine is found at equilibrium, calculate the value of equilibrium constant.

For the reaction
SrCO₃ (s) ⇌ SrO (s) + CO₂(g),
the value of equilibrium constant K_P = 2.2 x 10^–4 at 1002 K. Calculate K_C for the reaction.

To study the decomposition of hydrogen iodide, a student fills an evacuated 3 litre flask with 0.3 mol of HI gas and allows the reaction to proceed at 500^o C. At equilibrium he found the concentration of HI which is equal to 0.05 M. Calculate K_C and K_{P for this reaction.}