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Important Long Question Of Chemistry

 Important Long Question Of Chemistry class 11 NEB



Empiricel, Molecular Formula and Limiting Reactants

  1. 2 g of magnesium is burnt in a closed vessel containing 3 g of oxygen.
  • Which one is limiting reactant?
  • Calculate the mole of reactant left over.
  • How many gram of MgO are produced?
  • What is the mass of H2SO4 required to neutralize MgO formed in the reaction?

Avogadro's Hypothesis and Its Applications

  1. A trivalent metal oxide contains 31.6% of oxygen. What is the atomic mass of the metal?
  2. Apply Avogadro's Hypothesis to derive the relationship between vapour density and molecular mass of a gas. An oxide on nitrogen contains same of its own volume of nitrogen whose vapour density is 54. Determine the molecular formula of nitrogen oxide.
  3. How would you apply Avogadro's Hypothesis to show the molecular weight of gas is twice of its vapour density? An oxide of nitrogen contains same of its own volume of nitrogen and has vapour density equal to 22. Determine molecular formula of the nitrogen oxide.
  4. A divalent metal oxide contains 40% of oxygen. What is the atomic weight of metal?

State of matter

Gaseous State

  1. State Boyle's and Charle's Law. Derive PV=nRT. When 2 g of a gas (A) is introduced into an evacuated flask kept at 25° C, the pressure is found to be one atmosphere. If 3 g of another gas (B) is added to the same flask, the total pressure becomes 1.5 atmospheres at the same temperature. Assuming ideal behavior of gases. Calculate the ratio of molecular masses.
  2. State and explain Graham's law of diffusion. What are the application of Graham's law? Through the two ends of a glass tube of length 2 meters, hydrogenchloride (HCL) and ammonia (NH3) gases are allowed to enter. At what distance ammonium chloride will first appear?
  3. Write down the postulates of Kinetic molecular theory of gases. Why do gases show deviations form ideal behaviour at low temperature and high pressure? A saturated hydrocarbon having molecular formula CnH2n+2 diffusion through a porous membrane twice as fast as sulphur dioxide. Calculate the volume occupied by the hydrocarbon at 27° C and 2 atmospheric pressure.
  4. Distinguish between an ideal gas and a real gas. An evacuated glass vessel weights 50 g when empty, 148 g when filled with a liquid of density 0.98 g/cc and 50.5 g when filled with an ideal gas at 760 mm Hg at 27° C . Calculate the volume of the ideal gas STP.
  5. State Boyle's Law and derive P1V1 = P2V2. How would you justify Boyle's Law by graphical explanations?

Liquid State

  1. Write notes on solubility curve and its applications

Atomic Structure

  1. Explain main postulates of Bohr's theory of atomic model. How did this theory justify the origin of spectral lines in hydrogen atom?
  2. Describe Rutherford's nuclear model of an atom. Point out its limitations.
  3. What are the conclusions made by Rutherford's alpha-ray scattering experiments about the structure of atom. Point out the defect of this model.
  4. What are the differences between an atomic orbit and an atomic orbital? Draw the shapes of S and P orbitals.
  •  Discuss how Rutherford's nuclear model of an atom is introduced on the basis of alpha particular scattering experiment. Point out the limitation of the model.
  • How is the nuclear model of atom improved by Bohr's?
  • Why is Bohr's atomic model appeared to be defective in the light of Heisenberg's uncertainty principle ?

Write Short Notes On

  • Quantum numbers.

Electronic Theory Of Valency and Bonding

  1. Discuss the formation of potassium chloride and carbon tetrachloride molecules on the basis of electronic theory of valency. Give any two characteristics of ionic and covalent compounds.

Short Notes on

  1. Covalent bonding
  2. Resonance 

Periodic Classification Of Elements

  1. What is periodicity and its causes? How do atomic radii vary in a group and why?
  2. State Mendeleev's periodic law. What are the anomalies of Mendeleev's periodic table? How are these anomalies removed in modern periodic table?
  3. Define ionization energy? How do 'Nuclear charge' and size of the atom' influence the magnitude of the ionization energy? Ionization energy of 'N' is higher than that of 'O'. Give reason.

Short Notes On

  • Advantage of modern periodic table
  • Mendeleev's periodic table and its demerits
  • Characteristics of s,p,d and f blocks of elements
  • Modern periodic table
  • Periodic properties of elements 

Oxidation and Reduction

  1. Define reducing agent giving an example.Balance the following redox reaction by oxidation number or ion-electron method: 
MnO2 + HCL----->MnCl2 + Cl2 + H2O

2. Distinguish between oxidation and reduction. Balance the following equation by oxidation number or ion electron method.
N2H2 + ClO3 -----> NO + Cl + H2O

3. Define redox reaction. 'Oxidation and reduction is simultaneous process' explain.

4. Electronic interpretation of oxidation and reduction.

Equilibrium

  1. State Le-chatlier's principle. How does the change in temperature and pressure affect the equilibrium of the following reaction?                                      N2(g) + 3H2(g) <----->2NH3(g) + 22.4 K Cal
  2. Relationship between Kp and Kc
  3. Law of mass action and characteristic of equilibrium constant.
  4. Application of Le-chatelier's principle in chemical equilibrium.

Nitrogen and its compounds

  1. How is ammonia manufactured by haber's process? Write the action of ammonia on copper sulphate solution.
  2. How is Nitric acid from prepared from catalytic oxidation of ammonia?
  3. Give the balance chemical equation for the preparation of ammonia from nitrogen and hydrogen. How does ammonia reacts with:.                                 i) Mercurous paper.    ii) Oxygen.             iii) Nessler's reagent.  iv) Sodium metal
  4. Write down the principle and procedure with self-explanatory diagram for the manufacture of nitric acid by catalytic oxidation of ammonia. How does Conc. HNO3 react with:.           i) KI.                      ii) Zn.                                explain why ?                                              i) Conc. HNO3 is stored in dark bottle.     ii) Iron becomes passive when treated with Conc. HNO3
  5. How is ammonia manufactured by Haber's process? What happens when ammonia is passed through.                      i) Copper sulphate solution.                       ii) Heated copper oxide.                             Give reaction for the conversation of ammonia to nitric acid.
  6. Describe the manufacture of nitric acid by catalytic oxidation of ammonia. Write a chemical reaction to show nitric acid contains nitrogen.
  7. Describe the manufacture of nitric acid by Ostwald's process giving a neat and labelled diagram. How is nitric acid detected in the laboratory?

Non metals II

Hallogens:

  1. Why can't HBr and HI be prepared by heating Conc.H2SO4 with bromide and iodide respectively? Write down correct reactions to prepare them. How would you test the presence of Br -ions in its aqueous solution?
  2. Explain, How the bromine is manufacture from Carnallite? What happens when Br2 reacts with hot and conc.NaOH solution ?
  3. Give balanced chemical reaction of the preparation of chlorine in the laboratory. Compare the bleaching action of CL2 and SO2.
  4. Why can't HI be prepared by using Nal and Conc.H2SO4 ? Give the balance chemical reaction for the preparation of HCL . How would you test the presence of CL- and Br- in its aqueous solution ?
  5. Give the balance chemical reaction of HCL and HBr  in the laboratory. How would you test the presence of CL- ,Br- and I- ion in its solution?
  6. What is Carnallite? How is bromine manufactured from Carnallite? Give the action of Br2 on hot NaOH.
  7. Write down the principle for the preparation of hydroiodic acid (HI) in laboratory. How does HI react with MnO2 and CuSO4 .

Carbon:

  1. How is carbon monoxide prepared from oxalic acid in the laboratory ? Give its action with heated nickel.
  2. What happen when :
  • Carbon monoxide is passed over finelly divided nickel at 80 degree c
  • a gas obtained from a mixture of marble and dilute hydrocholoric acid is passed into lime water till excess.
  • a gas obtained from a mixture of copper turnings and hot conc.Sulphuric acid is passed into chlorine water.
  • Carbon monoxide is passed over finely divided nickel.
     3. Define allotropy? Show that diamond and graphite consist of carbon only.
     4. Write short notes on:
  • Graphite
  • Allotropes of carbon
  • Fullerenes
  • Amorphous forms



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