33. Purification and analysis of organic compounds
34. Nomenclature of Organic compounds
35. Reaction Mechanisms
36. Hydrocarbons
37. Haloalkanes (Alkyl halides)
38. Alcohol, Phenol and Ether
39. Aldehyde and Ketones
40. Carboxylic acids
41. Compounds conatining Nitrogen
42. Polymers
43. Chemistry in daily life
44
Physical chemistry
7. Chemical equilibrium
1. For the reaction N2 + O2 ⇌ 2NO, the equilibrium constant Kc changes with the change in
[MOE Model, MOE 2008]
Total pressure
Amount of NO
Amount of N2 and O2
Temperature
(d) Equilibrium constant (Kc) only changes with temperature for a given reaction.
2. In the given reaction, which one favors the formation of product? 2SO2 + O2 ⇌ 2SO3, ΔH = -ve
Decrease in pressure
Increase in pressure
Increase in concentration of SO2
Increase in temperature
(b) Forward reaction has fewer moles of gas (3→2) and is exothermic - favored by high pressure and low temp.
3. The synthesis of ammonia from Nitrogen and hydrogen proceeds with a decrease in volume, this reaction will be favored by
[MOE 2064]
Decrease in pressure
Increase in pressure
Unaffected by pressure
Addition of ammonia
(b) N2 + 3H2 ⇌ 2NH3 (4→2 moles gas) - Le Chatelier's principle favors high pressure.
4. According to Le-Chatelier's principle, which of the following shifts the reaction of Haber's process for formation of NH3 to right side?
[MOE 2003, MOE 2062]
Concentration of H2 is decreased
Temperature is increased
Pressure is increased
Pressure is decreased
(c) N2 + 3H2 ⇌ 2NH3 favors product side with increased pressure (fewer gas moles).
5. Which of the following expression represents the solubility product (Ksp) of lead (II) chloride?
[MOE 2063]
[Pb2+][Cl-]
[Pb2+] + [2Cl-]
[Pb2+][Cl-]2
[Pb2+][Cl2]
(c) For PbCl2 ⇌ Pb2+ + 2Cl-, Ksp = [Pb2+][Cl-]2
6. At equilibrium: equilibrium constant of a reaction is not affected by
[MOE 2058]
Temperature
Catalyst
Concentration of reactant
Concentration of product
(b) Catalyst speeds up both forward and reverse reactions equally, not affecting Keq.
7. For A + 2B ⇌ 2C + D: 1.1 mole of A combines with 2.2 moles of B at equilibrium and 0.2 moles of C is produced, then the value of equilibrium constant will be
8. Le-Chatelier's principle was applicable to the following reaction, when temperature increases, reaction shifts to the right, then the reaction will be
9. Ethyl alcohol and acetic acid are mixed in equimolar proportion; equilibrium is attained when 2/3 of the acid and alcohol are consumed. The equilibrium constant of the reaction will be
11. If 'a' moles of N2O4 confined in a volume 'V' undergoes dissociation and 'x' moles dissociate at equilibrium, then the dissociation constant 'K' will be given by
[IOM 2008]
x2/(a-x)V
4x2/(a-2x)V
2x2/(a-x)V
x/(a-2x)
(b) For N2O4 ⇌ 2NO2, K = [NO2]2/[N2O4] = (2x/V)2/((a-x)/V) = 4x2/(a-x)V
12. The equilibrium constant for the reaction, 2NH3 ⇌ N2 + 3H2, is 6 × 10-3. The equilibrium constant for the reverse reaction N2 + 3H2 ⇌ 2NH3 will be