DGK. Board 2016
Annual
Group-1
INTERMEDIATE PART-1
11^th Class
Chemistry paper
Time Allowed: 20 Minutes
Marks:17

• 27 g AL will react completely with how mass of O₂ to produce Al₂O_3:

1. 8 g of oxygen
2. 16 g of oxygen
3. 32 g of oxygen
4. 24 g of oxygen

• The number of moles of CO₂ which contain 8.0 gm of oxygen:

1. 0.25
2. 0.50
3. 1.0
4. 1.50

• Solvent extraction is an equilibrium process and it is controlled by:

1. Law of mass action
2. the amount of solvent
3. Distribution law
4. The amount of solute

• The molar volume of CO₂ is maximum at:

1. S.T.P
2. 127⁰ C and I atm
3. 0⁰C and 2 atm
4. 273⁰C and atm

• The order of the rate of diffusion of gases NH₃ SO₂ CL₂ and CO₂  is:

1. NH₃>SO₂> CO₂
2. NH₃>CO₂ > SO₂> CL₂
3. CL₂> SO₂> CO₂> NH₃
4. NH₃> CO₂> CL₂> SO₂

• In order to mention the boiling point of water at 110⁰C, the external pressure should be:

1. Between 760 Torr and 1200 Torr
2. Between 200 Torr and 760 Torr
3. 765 Torr
4. Any value of pressure

• Which of the following is psendo solid:

1. CAF₂
2. Glass
3. NaCl
4. Iron

• Bohr model of atom is contradicted by:

1. Planck,s quantum theory 
2. Dual nature matter
3. Heisenberg,s un-certain principle
4. Ruther ford atomic model

• Ruther ford,s model failed because

1. The atomic did not have a nucleus and electrons
2. It did not account for the attraction between electrons and protons
3. It did not account for the stability of the atom
4. There is no space between nucleus and the electrons

• Which of the following species has unpaired electrons in anti bonding molecular orbits:

1. O²⁺₂
2. N₂^2-
3. B₂
4. F₂

• The number of bonds in nitrogen molecule is

1. One σ and π
2. One σ and two π
3. Three sigma only
4. Two σ and one π

• The change in heat energy of a chemical reaction at temperature and reassure is called:

1. Enthalpy change
2. Heat of sublimation
3. Bond
4. Internal energy change

• The pH of 10^-3 moil dm^-3 of an aqueous solution of H₂ SO₄ is:

1. 3.0
2. 2.7
3. 2.0
4. 1.5

• For which system does the equilibrium constant “KC” has units of (concentration):

1. 2N₂+3H₂ 2NH₃
2. H₂+l₂ 2Hl
3. 2NO₂ N₂O₄
4. 2HL H₂ + F₂

• A solution of Glucose is 10% w/y. The volume in which I gm mole of it is dissolved will be:

1. 1 dm³
2. 1.8 dm³
3. 200Cm³
4. 900Cm³

• If the salt bridge is not used between two half cells, then the voltage:

1. Decrease rapidly
2. Decrease slowly
3. Does not change
4. Drops to zero

• The unit of the rate constant bis the same as that of the rate of reaction in:

1. First order reaction
2. Second order reaction
3. Zero order reaction
4. Third order reaction

DGK. Board 2016
Group-I
INTERMEDIATE PART-1
11^th Class
Chemistry
paper-1
Time Allowed: 2:40 Hours
Marks: 68
Section-I

Q.2 Attempt any eight parts

(i) What are isotopes? Why they have same chemical properties?
(ii) Write two stolchiometric assumption.
(iii) Define molecular formula. How it is related to empirical formula?
(iv) Mention the major steps involved in crystallization.
(v) Write down any two application of chromatography?
(vi) Why water vapor do not behave ideally at 273 K?
(vii) Why real gases deviate from ideal behavior?
(viii) Write two uses of plasma.
(ix) What are the buffer solution? How an acidic buffer is prepared?
(x) Define pH and pOH with mathematical expressions.
(xi) Calculate the percentage by weight of NaCL , if 2 g of NaCL is dissolved in 20 g of water.
(xii) What is parts per million? Write its mathematical expression.

Q.3 Attempt any eight parts 8×2=12

(i) What is the effect of intermolecular forces on vapor pressure?
(ii) Write two advantages of vacuum distillation.
(iii) Define allotropy. Give its one example.
(iv) Cathode rays posses momentum justify it.
(v) Write four properties of molecular solids.
(vi) Give two defect of Bohr,s atomic model.
(vii) Differentiate between line spectrum and continuous spectrum.
(viii) Define Aufbau principle and pual,s Exclusion principle.
(ix) What is solubility curve? Name its two types.
(x) Calculate the oxidation number of chromium in K₂CrO₄
(xi) How is lead accumulator recharged?
(xii) What is function of salt bridge in voltaic cell?

Q.4 Attempt any eight parts 6×2=12

(i) Why molecular orbit theory is superior to valence bond theory?
(ii) What is Expression to calculate the dipole moment of a molecule?
(iii) Write two main postulates of VSER theory.
(iv) Why the radius of Na ion is less than the atomic radius of NA atom?
(v) Differentiate between internal energy and enthalpy.
(vi) What do you mean by standard enthalpy of Atomization?
(vii) Write only names of two physical method for determining rate of a reaction.
(ix) What do you mean by active example of reaction?

Section-II

Q.5(A) A sample of liquid consisting of carbon, hydrogen and oxygen was subject to combustion, Analysis, 0.5439g of the compound gave 1.039 g of CO₂, 0.6369g of H₂O. of H₂O. Determine the empirical formulas of the compound.
(B) What is the effect of external pressure on boiling point of a substance? Give example.

Q.6(A) Drive an expression from general gas equation to calculate the density of a gas.
(B) Write J.J Thomson method to measure the e\m value of electron.

Q.7(A) Define enthalpy and power q_p = 𝝙ll
(B) Define hybridization. Explain the geometry of ethane on the basis of sp² hybridization.

Q.8(A) Ca(OH)₂ is a sparingly soluble compound its solubility product is 6.5 × 10^-6. Calculate the Solubility of Ca(OH)₂.
(B) Describe the constriction and working of standard hydrogen electrode (SHE)

Q.9(A) Explain positive and negative deviation of non-ideal solution.
(b) Write four industrial application of Electrolysis.

DGK.Board 2016
(Annual) Group-II
INTERMEDIATE PART-1
11^TH CLASS
CHEMISTRY
PAPER- I
Time Allowed: 20 Minutes
Mark: 17

• During combustion analysis, CO₂ produced is absorbed in:

1. Mg(ClO)₂
2. 50% KOH
3. CaCl₂
4. P₂O₅

• The largest number of molecules is present in:

1. 3.6g
2. 4.8g of C₂H₅OH
3. 2.8 g of CO
4. 5.4g of N₂O₅

• Solvent extraction method is particularly useful technique for separation when the product to be separation is:

1. Non- volatile or thermally unstable
2. volatile or thermally unstable
3. Non-volatile or thermally stable
4. volatile or thermally unstable

• Which of the following will have the same number of molecules at STP:

1. 280cm³ of CO₂ and 280cm³ of N₂O
2. 11.2 dm³ of O₂ and 32g of O₂
3. 44g of CO₂ and 11.2dm³ of CO
4. 28g of N₂ amd 5.6 dm³ of O₂

• The deviation of gas from ideal behavior is maximum at:

1. -10⁰C and 5.0 atm
2. -10⁰C and 2.0 atm
3. 100⁰C and 2.0 atm
4. 0⁰C and 2.0 atm

• London dispersion forces are the only forces present amount at:

1. Molecules of water in liquid state
2. Atoms of helium in gaseous state at high temperature
3. Molecules of solid iodine
4. Molecules of hydrogen chloride

• Ionic solids are characterized by:

1. Low melting point
2. Good conductive in solid state
3. High vapor pressure
4. Solubility in polar solvent

• Bohr model of atom was contradicted by:

1. Plank,s quantum theory
2. Dual nature of matter
3. |Heisenberg,s uncertainty principle
4. Aufbua principle

• When 6d orbital is complete, the entering electron goes into:

1. 7f
2. 7s
3. 7p
4. 7d

• The excrementally determined bond angle in NH₃ is:

1. 109.5⁰
2. 107.5⁰
3. 104.5⁰
4. 102.5⁰

• Which of the following is zero dipole moment?

1. NH₃
2. CHCl₃
3. H₂O
4. BF₃

• For the reaction of NaOH + HCl→ Nacl + H₂O the change in enthalpy is called.

1. Heat of reaction
2. Heat of formation
3. Heat of neutralization
4. Heat of combustion

• The pH of human blood is maintaind at pH:

1. 7.30
2. 7.35
3. 7.00
4. 8.00

• An excess of aqueous siver nitrate is added to aqueous barium chloride and precipitate is removed by:

1. Ag⁺ and NO^- only
2. Ag⁺ amd Ba²⁺ and NO^-₃
3. BA^- and NO^-₃ only
4. BA²⁺ , NO^-₃ and Cl^-

• The molal boiling point constant is the ratio of the elevation in boiling point to:

1. Molarity
2. Molality
3. Mole fraction of solvent
4. Mole fraction of solute

• If the salt bridge is not used between half cell, then the voltage

1. Decrease rapidly
2. Decrease slowly
3. Does not change
4. Drops to zero

• The rate of reaction:

1. Increase as the reaction proceeds
2. Decrease as the reaction proceeds
3. Remain the same as the reaction proceeds.
4. May decrease or increase as the reaction proceeds

DGK. Board 2016
(Annual) Group-II
INTERMEDIATE PART-1
11^TH CLASS
CHEMISTRY
PAPER- I
Time Alowed:2:40 Minutes
Mark: 68

Q.2Attempt any eight parts

(i) Define Avogadr,s Number with two example.
(ii) Define Stoichiometrions.
(iii) Prove that N₂ and CO have the same number of electrons. Protons and neutrons.
(iv) How undesireable colors are removed from the crystals?
(v) Define the method of drying of the crystallized substance.
(vi) Define Avogadro,s law with two suitable example.
(vii) Why do we feel comfortable in expressing the densities of gases in the units of g\dm³ rather than g\cm³.
(viii) Define critical temperature and critical pressure, giving one example in each case.
(ix) Define effect of catalyst on equilibrium constant.
(x) Calculate pH of10^-4 mol dm^-3 of Ba(OH)_2.
(xi) The concentration in term of molality is independent odf temperature but molarity depend upon temperature. Justify it.
(xii) Justify that boiling point of solvent increase due to the presence of solutes.

Q.3Attempt any eight parts 8×2=16

(i) Define transition temperature with two examples.
(ii) Water is liquid in room temperature, while H₂S is a gas. Explain.
(iii) Give reason that ice float on water.
(iv) Explain cleavage of the crystal and cleavage plan.
(v) State Hund,s rule.
(vi) How neutron are used in the treatment of the cancer.
(vii) What is Lyman series?
(viii) Write four properties of cathode rays.
(ix) Define hydration and hydrolysis.
(x) What is standard electrode potential.
(xi) Define electrolytic cell. Give example.
(xii) Write functions of salt bridge.

Q.4Attempt any six parts 6×2=12

(i) The depole moment of CO₂ and CS₂ are zero, but that of SO₄ is 1.61 D. justify.
(ii) Sketch of molecular orbit picture of π (2p₂) and π* (2p₂) of N₂ molecule.
(iii) Why the abnormality of bond length is Hl is less prominent than that of HCl.
(iv) Write the name of factor effecting the strength of a bond.
(v) Define Enthaply of formation with one example.
(vi) Differentiate between internal energy change and enthalpy|?
(vii) Define order of reaction with one example.
(viii) Justify that rate of reaction depend upon surface area give one example also.
(ix) Define Hetrogeneous catalysis with one example.

Section-II

Q.5(A) A sample of liquid consisting of carbon, hydrogen and oxygen was subject to combustion analysis.0.5439 g of the compound gave 1.039 g of CO₂, 0.369 g Of H₂O. Determine the empirical formula of the compound.
(B) Define covalent solid with example. Write four properties of covalent solid.

Q.6(A) State and explain Graham,s law of diffucion.
(b) What is spectrum? Explain Atomic Emission and atomic absorption spectrum.

Q.7(A) Explain postulates of molecules orbital theory.
(b) Explain Glass calorimetric method for the measurement of Enyhalpy of reaction.

Q.8(A) Calculate the pH of buffer solution in wich 0.11 molar CH₃COONa and 0.09 molar Acetic acid solution are present Ka for acetic acid is 1.85 × 10.5^-5 .
(b) How does Arrehenius equation help us to calculate the energy of activation of a Reaction.

Q.9(A) Write four differences between idea and non-ideal solution.
(B) Describe the standard hydrogen electrode with diagram.