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Punjab (PTB) · Quarter book test · Free

1st Year Chemistry 3rd Quarter Book Paper

40 marks · 1 hour · 28 questions. Covers: 4 chapters (CHAP 9: Acid-Base Chemistry to CHAP 12: Nitrogen and Sulfur).

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1st Year Chemistry 3rd Quarter Book Paper

1st Year · Chemistry · Punjab (PTB)

Name: ____________Roll No: ________Class/Section: ________Date: ________Total marks: 40Time: 1 hour

Q1. Multiple choice questions (Attempt all · 12 × 1 = 12)

  1. n-Butanol and diethyl ether are:

    1. Geometrical isomers

    2. Position isomers

    3. Chain isomers

    4. Functional group isomers

  2. Nitrosomonas helps in conversion of:

    1. NO4- to NO2-

    2. NO4+ to NO2-

    3. NO4- to N2

    4. N2 to NO3-

  3. For the half-reaction if the concentration of , if the concentration of M n + ions is decreased below 1 M at 298 K, how will the actual electrode potential (E) change? 

    1. E will become more positive

    2. E will remain unchanged

    3. E will become less positive (or more negative)

    4. E will always become 0 V

  4. The pH of 10-3mol dm-3 of an aqueous solution of H2SO4 is:

    1. 3.0

    2. 2.7

    3. 2.0

    4. 1.5

  5. In Ethene, each carbon atom is:

    1. Sp3 hybridized

    2. Sp2-hybridized

    3. Sp-hybridized

    4. Unhybridized

  6. The role of vanadium(V) oxide (V2O5) in the Contact Process is:

    1. Purifying gas

    2. Absorbing water

    3. Acting as catalyst

    4. Neutralizing acid

  7. 1 Faraday of electricity deposits:

    1. 1 mole of electrons

    2. 6.022 × 1023 electrons

    3. 1 gram of any metal

    4. Equivalent mass of a substance

  8. A basic buffer solution can be prepared by mixing:

    1. Weak acid and its salt with strong base

    2. Strong acid and its salt with weak base

    3. Weak base and its salt with strong acid.

    4. Strong base and its slat with weak acid

  9. Intermediate cyclic stage formed during the addition of bromine into ethene is:

    1. Bromide ion

    2. Bromonium ion

    3. Bromine

    4. Viccinal dibromide

  10. Vehicles tested near a smog-prone area show higher emissions of:

    1. O2 and H2

    2. NO and NO2

    3. H2O and CO2only

    4. Argon and helium

  11. Eo values help us to determine:

    1. Atomic number

    2. Color of elements

    3. The ease of redox reactions

    4. Boiling points

  12. The ionic product of water will increase if:

    1. H+ ions are added,

    2. OH- ions are added

    3. Temperature is increased

    4. H+ and OH- ions are added in equal amount

Q2. Short questions (Attempt any 8 of 12 · 8 × 2 = 16)

  1. Why electrode potential of Cu is called reduction potential?

  2. Give an example of a sulfur-containing fragrance compound and its application.

  3. Write down name of the following compounds according to IUPAC-System. (i) CH2=CH-CH=CH2 (ii)CH2=C-CH2CH2CH3 (image) (iii) (CH2CH2)3CH

  4. Why is the water molecule considered amphoteric according to the Bronsted-Lowry theory? Provide equations to illustrate its behavior as both an acid and a base.

  5. State the value of Avogadro's constant and Faraday's constant.

  6. How does V2O5 catalyze the formation of SO3?

  7. Differentiate between open and closed chain hydrocarbons.

  8. Explain the concept of a conjugate acid-base pair using a specific example.

  9. What is electrolysis?

  10. What percentage of sulphuric acid is used in fertilizers?

  11. Give the structures of (i) butane and isobutane, (ii) isopentane and neopentane.

  12. Define the following with an example for each:(i) Common ion effect (ii) Acid-base Indicator

Q3. Long questions (Attempt any 3 of 4 · 3 × 4 = 12)

  1. Describe the free radical halogenation of methane using Cl2 as an example.

  2. Calculate the electrode potential for a zinc electrode immersed in a 0.010 mol dm-3 solution of zinc sulfate (ZnSO4) at 298 K. The standard electrode potential (E°) for is -0.76 V. (Gas constant, R = 8.31JK-1mol-1,Faraday constant, F = 96500C mol-1)

  3. Describe the position of nitrogen in the periodic table, its physical properties and laboratory preparation. Why nitrogen is least reactive compounds with highest relative abundance?

  4. Derive the relation for the calculation of the ionization constant for acids.