Rawalpindi BOARD
(Inter Part-I Class 11th)
Session (2019)
Time: 20 minutes
Marks: 17
Objective
Note:
- You have choices for each objective-type question as A, B, C, and D.
- The choice which you think is correct, fill that circle in front of that question number with a marker or pen.
- Cutting or filling two or more circles will result in zero marks for that question.
Q.1: Answer all the following Multiple Choice Questions.
- An aqueous solution of ethanol in water has vapour pressure:
A) equal to that of water
B) equal to that of ethanol
C) more than the sum of mole fractions
D) less than that of water
- The sum of mole fractions of gases in a mixture is:
A) always more than one
B) always less than one
C) always one
D) may be less or more than one
- Stronger the oxidizing agent, the greater the:
A) Oxidation potential
B) Reduction potential
C) Redox potential
D) E.M.F of the cell
- The rate of reaction:
A) Increases as the reaction proceeds
B) Remains the same as the reaction proceeds
C) May decrease or increase as the reaction proceeds
D) Remains unchanged
- 27 g of Al will react completely with how much mass of O₂ to produce Al₂O₃?
A) 8 g of oxygen
B) 16 g of oxygen
C) 32 g of oxygen
D) 24 g of oxygen
- The number of moles of CO₂ which contain 8.0 g of oxygen is:
A) 0.25
B) 0.50
C) 1.0
D) 1.50
- Solvent extraction method is a useful technique for separation when the product to be separated is:
A) Non-volatile or thermally unstable
B) Volatile or thermally unstable
C) Non-volatile or thermally stable
D) Volatile or thermally stable
- At constant pressure, at what temperature will the volume of a gas become twice of what it is at 0°C?
A) 546°C
B) 200°C
C) 546 K
D) 273 K
- Amorphous solids:
A) Have a sharp melting point
B) Undergo clean cleavage when cut with a knife
C) Have a perfect arrangement of atoms
D) Can possess small regions of orderly arrangement of atoms
- London dispersion forces are the only forces present among:
A) Molecules of water in liquid state
B) Atoms of helium in gaseous state at high temperature
C) Molecules of solid iodine
D) Molecules of hydrogen chloride gas
- The nature of positive rays depends on:
A) The nature of the electrode
B) The nature of the discharge tube
C) The nature of the residual gas
D) The nature of the voltage applied
- The wave number of the light emitted by a certain source is 2×10⁶ m⁻¹. The wavelength of this light will be:
A) (Missing data)
B) (Missing data)
C) (Missing data)
D) (Missing data)
- Which of the following molecules has a zero dipole moment?
A) CO₂
B) H₂O
C) CH₄
D) NH₃
- Which of the hydrogen halides has the highest percentage of ionic character?
A) HF
B) HCl
C) HBr
D) HI
- In an endothermic reaction, the heat content of the:
A) Product is more than that of reactants
B) Reactants is more than that of products
C) Both A and B
D) Reactants and products are equal
- The solubility product of AgCl is 2×10⁻¹⁰ mol²/dm⁶. The maximum concentration of Ag⁺ ion in the solution is:
A) 2×10⁻⁵ mol/dm³
B) 1.41×10⁻⁵ mol/dm³
C) 1.0×10⁻¹⁰ mol/dm³
D) 4.0×10⁻²⁰ mol/dm³
- The relationship between Kp and Kc is given by:
A) Kp = Kc(P)ⁿ
B) Kp = Kc
C) Kp = Kc(RT)ⁿ
D) Kp = Kc/(RT)
RAWALPINDI BOARD
Chemistry (New Scheme)
(Inter Part-I Class 11th)
Time: 2:40 Hours
Marks: 68
Note:
- Section I is compulsory.
- Attempt any three questions from Section II.
Section I: (Compulsory)
Q.2: Write short answers to any eight of the following parts.
- Discuss the purification of sodium chloride by the common ion effect.
- Write down the role of a magnetic separator in a mass spectrometer.
- Define molecular formula and empirical formula. Give the relationship between them.
- Write down Kc for the following reaction, assuming the volume of the reaction mixture is at equilibrium:
PCl₅ ⇌ PCl₃ + Cl₂ - How do you justify that the greater quantity of sodium acetate (CH₃COONa) in acetic acid decreases the dissociation power of acetic acid, thus increasing the pH?
- Explain the respiration process in the light of Dalton’s Law of partial pressure.
- Convert -40°C into the Fahrenheit scale.
- Derive Charles’s law from the kinetic theory of gases.
- Define pH and pOH. What is the sum of pH and pOH?
- What are molecular ions, and how are they produced?
- How is undesirable color removed from the crystals?
- Define sublimation with examples.
Section II:
Q.3: Write short answers to any eight of the following parts.
- Justify that a one-molal solution of urea in water is more dilute than its molar solution.
- What is meant by symmetry? Give elements of symmetry.
- Define colligative properties. Name some important colligative properties.
- What is the octet rule? Give two examples of compounds that deviate from it.
- A freshly cut metal has a shiny look. Justify it.
- What factors influence electron affinity?
- No bond in chemistry is 100% ionic. Justify this statement.
- Why is the molecule of BF₃ triangular planar?
- What is meant by a state function? Give an example.
- Differentiate between internal energy and enthalpy.
- Define crystal and crystallite.
- What is the habit of a crystal? Give one example.
Q.4: Write short answers to any six of the following parts.
- State Moseley’s law.
- What is Hund’s rule?
- How is the atomic emission spectrum obtained?
- Why are positive rays also called canal rays?
- What is Electrochemistry?
- Give advantages of a fuel cell.
- What is a zero-order reaction? Give an example.
- Write two characteristics of a catalyst.
- Calculate the oxidation state of Cr in:
a) Cr₂(SO₄)₃
Section III: (Attempt any three questions)
Q.5:
a) The combustion analysis of an organic compound shows it contains 65.44% carbon, 5.50% hydrogen, and 29.6% oxygen. What is the empirical formula of the compound if the molar mass is 110.15 g/mol? Calculate the molecular formula.
b) Discuss the manometric method for the measurement of the vapor pressure of a liquid.
Q.6:
a) State and explain Graham’s Law of diffusion.
b) State and explain Planck’s quantum theory.
Q.7:
a) Describe the structure of NH₃ and H₂O with the help of atomic orbital hybridization.
b) Describe Hess’s Law of constant heat summation with two examples.
Q.8:
a) Derive the Henderson equation for acidic and basic buffers.
b) What is electrolysis? Discuss the electrolysis of fused salt PbBr₂.
Q.9:
a) The vapor pressure of water at 30°C is 28.4 torr. Calculate the vapor pressure of a solution containing 70.0 g of cane sugar (C₁₂H₂₂O₁₁) in 1000.0 g of water at the same temperature. Also, calculate the lowering of the vapor pressure.
b) How does the Arrhenius equation help in calculating the energy of activation of a reaction?