State the first law of thermodynamics.

Define Hess's law of constant heat summation.

Explain intensive properties with two examples

What is the usual definition of entropy? What is the unit of entropy?

Predict the feasibility of a reaction when
(i) both ΔH and ΔS positive
(ii) both ΔH and ΔS negative
(iii) ΔH decreases but ΔS increases

Define Gibb's free energy.

Define enthalpy of combustion.

State the third law of thermodynamics.

Identify the state and path function out of the following:
a) Enthalpy
b) Entropy
c) Heat
d) Temperature
e) Work
f) Free energy.

For the equilibrium PCI₅(s) ⇌ PCl₃(g) + CI₂(g) at 25°C k_c = 1.8 x 10^-7 R = 8.314 Jk^-1 mol-¹ Calculate ΔG^o for the reaction.

Calculate the entropy change in surroundings when 1 mol of H₂0_(I) is formed under standard conditions. Given \(\Delta { H }^{ \ominus }\) = - 286 kJ mol^-1.

Define Zeroth law of thermodynamics (or) Law of thermal equilibrium.

What are spontaneous reaction? Give three examples for spontaneous reaction.

Predict in which of the following, entropy increases or decreases.
(I) A liquid crystallizes into a solid
(ii) Temperature of a crystallized solid is raised from 0 K to 115 K
(iii) 2NaHCO_{3 (s)} \(\longrightarrow\) Na₂CO_{3 (s)} + CO_{2 (g)} + H₂O _(g)
(iv) H_{2 (g)} \(\longrightarrow\) 2H_(g)

What is meant by open system? Give example.

If there is no change in concentration, why is the equilibrium state considered dynamic?

For a gaseous homogeneous reaction at equilibrium, number of moles of products are greater than the number of moles of reactants. Is K_C is larger or smaller than K_P.

When the numerical value of the reaction quotient (Q) is greater than the equilibrium constant (K), in which direction does the reaction proceed to reach equilibrium?

Consider the following reactions,
H₂(g) + I₂(g) ⇌ 2 HI(g)
In each of the above reaction find out whether you have to increase (or) decrease the volume to increase the yield of the product.

State law of mass action.

Explain how will you predict the direction of a equilibrium reaction.

Derive a general expression for the equilibrium constant K_P and K_C for the reaction 
3H₂(g) + N₂(g) ⇌ 2NH₃(g).

Write a balanced chemical equation for  equilibrium reaction for which the equilibrium constant is given by expression
\(K_c={[NH_3]^4[O_2]^5\over [NO]^4[H_2O]^6}\)

Derive the relation between K_P and K_C.

Deduce the Vant Hoff equation.