NEET Chemistry Gaseous State MCQs Set E

Refer to NEET Chemistry Gaseous State MCQs Set E provided below available for download in Pdf. The MCQ Questions for Full Syllabus Chemistry with answers are aligned as per the latest syllabus and exam pattern suggested by NEET, NCERT and KVS. Multiple Choice Questions for Gaseous State are an important part of exams for Full Syllabus Chemistry and if practiced properly can help you to improve your understanding and get higher marks. Refer to more Chapter-wise MCQs for NEET Full Syllabus Chemistry and also download more latest study material for all subjects

MCQ for Full Syllabus Chemistry Gaseous State

Full Syllabus Chemistry students should refer to the following multiple-choice questions with answers for Gaseous State in Full Syllabus.

Gaseous State MCQ Questions Full Syllabus Chemistry with Answers

Question. A cylinder of capacity 20 litres is filled with H2 gas. The total average kinetic energy of translatory motion of its molecules is1.5x105 J.The pressure of hydrogen in the cylinder is:
a. 2×106 N /m2
b. 3×106 N /m2
c. 4×106 N /m2
d. 5×106 N /m2
Answer : D

Question. A gas at a certain volume and temperature has pressure 75 cm. If the mass of the gas is doubled at the same volume and temperature, its new pressure is:
a. 37.5 cm
b. 75 cm
c. 150 cm
d. 300 cm
Answer : C

Question. If 20 cm3 gas at 1 atm. is expanded to 50 cm3 at constant T, then what is the final pressure:
a. 20 x 1/50
b. 50 x 1/20
c.  1 x 1/20 x 50
d. None of these
Answer : A

Question. 400 cm3 of oxygen a 27°C were cooled to –3°C without change in pressure. The contraction in volume will be:
a. 40 cm3
b. 30 cm3
c. 44.4 cm3
d. 360 cm3
Answer : A

Question. How many moles of He gas occupy 22.4 litres at 30°C and one atmospheric pressure?
a. 0.90
b. 1.11
c. 0.11
d. 1.0
Answer : A

Question. 16 g of oxygen and 3 g of hydrogen are mixed and kept at 760 mm pressure and 0°C. The total volume occupied by the mixture will be nearly:
a. 22.4 litres
b. 33.6 litres
c. 448 litres
d. 44800 ml
Answer : D

Question. At room temperature, the rms speed of the molecules of certain diatomic gas is found to be 1930 m/s. The gas is:
a. H2
b. F2
c. O2
d. Cl2
Answer : A

Question. Cooking gas containers are kept in a lorry moving with uniform speed. The temperature of the gas molecules inside will:
a. Increase
b. Decrease
c. Remain same
d. Decrease for some, while increase for others
Answer : C

Question. The speeds of 5 molecules of a gas (in arbitrary units) are as follows: 2, 3, 4, 5, 6. The root mean square speed for these molecules is:
a. 2.91
b. 3.52
c. 4.00
d. 4.24
Answer : D

Question. The molecules of a given mass of a gas have a rms velocity of 200m/sec at 27°C and 1.0 x 105 N/m2 pressure.
When the temperature is 127°C and pressure is 0.5 x 105 N/m2 , the rms velocity in m/sec will be:

a. 100√2/3
b. 100√2
c. 400/√3
d. None of these
Answer : C

Question. At which of the following temperature would the molecules of a gas have twice the average kinetic energy they have at 20°C?
a. 40°C
b. 80°C
c. 313°C
d. 586°C
Answer : C

Question. A vessel contains a mixture of one mole of oxygen and two moles of nitrogen at 300 K. The ratio of the average rotational kinetic energy per O2 molecule to that per Nmolecule is:
a. 1 : 1
b. 1 : 2
c. 2 : 1
d. Depends on the moments of inertia of the two molecules
Answer : A

Question. The average translational energy and the rms speed of molecules in a sample of oxygen gas at 300K are 6.12×10–21J and 484m/s respectively. The corresponding values at 600K are nearly: (assuming ideal gas behaviour)
a. 12.45 x 10 −21 J,968m/ s
b. 8.78 × 10 −21 J,684m/ s
c. 6.21 x 10 −21 J,968m/ s 
d. 12.42 x 10 −21 J,684m/ s 
Answer : D

Question. The temperature at which RMS velocity of SO2 molecules is half that of He molecules at 300K is:
a. 150 K
b. 600 K
c. 900 K
d. 1200 K
Answer : D

Question. The rms speed of 2 N molecules in a gas is u. If the temperature is doubled and the nitrogen molecules dissociate into nitrogen atoms, the rms speed becomes:
a. u / 2
b. 2u
c. 4u
d. 14u
Answer : B

Question. A gas at 27°C has a volume V and pressure P. On heating its pressure is doubled and volume becomes three times.
The resulting temperature of the gas will be:

a. 1800°C
b. 162°C
c. 1527°C
d. 600°C
Answer : C

Question. A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintain the temperature of the gas in the flask at 52°C and the pressure remaining the same is:
a. 2.5 g
b. 2.0 g
c. 1.5 g
d. 1.0 g
Answer : D

Question. If the value of molar gas constant is 8.3 J/mole-K, the n specific gas constant for hydrogen in J/mole-K will be:
a. 4.15
b. 8.3
c. 16.6
d. None of these
Answer : A

Question. At constant temperature on increasing the pressure of a gas by 5% will decrease its volume by:
a. 5%
b. 5.26%
c. 4.26%
d. 4.76%
Answer : D

Question. On 0°C pressure measured by barometer is 760 mm. What will be pressure on 100°C?
a. 760 mm
b. 730 mm
c. 780 mm
d. None of these
Answer : D

Question. A perfect gas at 27°C is heated at constant pressure to 327°C. If original volume of gas at 27°C is V then volume at 327°C is:
a. V
b. 3V
c. 2V
d. V/2
Answer : C

Question. A gas is filled in the cylinder shown in the figure. The two pistons are joined by a string. If the gas is heated, the pistons will:
a. Move towards left
b. Move towards right
c. Remain stationary
d. None of these
Answer : B

Question. The capacity of a vessel is 3 litres. It contains 6 gm oxygen, 8 gm nitrogen and 5 gm CO2 mixture at 27°C. If R = 8.31 J/mole × kelvin, then the pressure in the vessel in N/m2 will be: (approx.)
a. 5×105
b. 5×104
c. 106
d. 105
Answer : A

Question. A closed vessel contains 8g of oxygen and 7g of nitrogen. The total pressure is 10 atm at a given temperature. If now oxygen is absorbed by introducing a suitable absorbent the pressure of the remaining gas in atm will be:
a. 2 b. 10
c. 4 d. 5
Answer : D

Question. Temperature of an ideal gas is T K and average kinetic energy is E = 2.07 x 10-23 T Joule/molecule. Number of molecules in 1 litre gas at S.T.P. will be:
a. 2.68×1022
b. 2.68×1025
c. 2.68×1028
d. 1.68×1022
Answer : A

Question. The average kinetic energy per molecule of helium gas at temperature T is E and the molar gas constant is R, then Avogadro’s number is:
a. RT/2E 
b. 3RT/E
c. E/2RT
d. 3RT/2E
Answer : D

Question. Under which of the following conditions is the law PV = RT obeyed most closely by a real gas?

""NEET-Chemistry-Gaseous-State-MCQs-Set-E

a. High pressure and high temperature
b. Low pressure and low temperature
c. Low pressure and high temperature
d. High pressure and low temperature
Answer : C

Question. The equation of state of a gas is given by (P + aT2/V)V= (RT + b),where a, b, c and R are constants. The isotherms can be represented by P = AVm − BVn , where A and B depend only on temperature then?
a. m= −c and n = −1
b. m = c and n =1
c. m= −c and n =1
d. m = c and n = −1
Answer : A

Comprehension Based

Paragraph–I

Two gaseous molecules A and B are traveling towards each other. Let the mean free path of the molecule be σ and Z be the collision number with other molecules at pressure 1 atm.
Answer the following questions:

Question. The free path of a gas molecule is the distance:
a. Between the two opposite is the distance
b. That molecules travel in one second
c. Through which a molecule moves between two successive collisions
d. None of these
Answer : C

Question. If the mean free path is σ at 1 atm pressure, then its value at 5 atm pressure is:
a. 5σ
b. (2/5)σ
c. 5/σ
d. None
Answer : C

Question. If Z is the total number of collisions which a gas molecule registers with others per unit time under particular conditions, then the collision frequency of the gas containing N molecules per unit volume is:
a. Z/N
b. NZ
c. ZN
d. NZ/2
Answer : D

Question. If the collision frequency of a gas at 1 atm pressure is Z, then its collision frequency at 0.5 atm is:
a. 1.0 Z
b. 0.707 Z
c. 2 Z
d. 0.5 Z
Answer : B

Paragraph –II

The constant motion and high velocities of gas particles lead to some important practical consequences. One such consequence is that gases mix rapidly when they come in contact. Take the stopper off a bottle of perfume, for instance, and the odour will spread rapidly through the room as perfume molecules mix with the molecules in the air.
This mixing of different gases by random molecular motion and with frequent collision is called diffusion. A similar process in which gas molecules escape without collision through a tiny hole into a vacuum is called effusion. Both the processes follow Graham’s law which is mathematically put as r ∝ 1/ d. The average distance travelled by molecules between successive collisions is called mean free path.

Question. The stopcocks of the bulbs X (containing NH3) and Y (containing HCl), both under identical conditions, are opened simultaneously. White fumes of NH4Cl are formed at point B. If AB = 36.5cm, then BC is approximately:

""NEET-Chemistry-Gaseous-State-MCQs-Set-E-1

a. 18.0 cm
b. 25.0 cm
c. 20.0 cm
d. 36.5 cm
Answer : B

Question. Select the incorrect statement (s).
a. The larger the size of the molecules, the smaller the mean free path
b. The greater the number of molecules per unit volume, smaller the mean free path
c. The larger the temperature, the larger the mean free path 
d. The larger the temperature, the smaller the mean free path
Answer : A

Question. X mL Heffuses through a hole in a container in 5 s. The time taken for the effusion of the same volume of the gas specified below under identical condition is:
a. 10 s : He
b. 20 s : O2
c. 25 s : CO
d. 55 g : CO2
Answer : B

Question. When CO2 under high pressure is released from a fire extinguisher, particles of solid CO2 are formed, despite the low sublimation temperature (–77ºC) at 1 atm because?
a. The gas does work pushing back the atmosphere using kinetic energy of molecules and thus lowering the temperature
b. The volume of the gas is decreased rapidly, hence, temperature is lowered
c. Both (a) and (b) are correct reasons
d. Neither (a) nor (b) is the correct reason
Answer : A

Question. Match the items of columns I and II:

Column IColumn II
(A) Critical temperature1. Gas can be liquefied
(B) Boyle’s temperature2. Deviate from ideal gas equation
(C) Compressibility factor (Z) < 13. Gas follows the ideal gas equation
(D) High temperature and low pressure4. Assumption of no intermolecular force of attraction is valid

a. A → 1; B → 2; C → 3; D → 4
b. A → 1; B → 3; C → 2; D → 4
c. A → 3; B → 2; C → 1; D → 4
d. A → 2; B → 1; C → 4; D → 3
Answer : B

Question. Match the items of columns I and II:

Column IColumn II
(A) Attractive tendency dominate1. Z = 3/8
(B) At Boyle’s temperature in
the high pressure region
2. Z < 1
(C) For a gas at very low pressure and at very high temperature3. Z > 1
(D) At the critical point4. Z = 1

a. A→ 1; B→ 2; C→ 3; D → 4
b. A→ 2; B→ 3; C→ 4; D → 1
c. A→ 3; B→ 2; C→ 1; D → 4
d. A→ 2; B→ 1; C→ 4; D → 3
Answer : B

Comprehension Based

Paragraph –I

Mean free path of molecule is the average distance traveled by a molecule between two successive collisions and is given by λ = 1/√2πd2 n where d is diameter of gas molecules, n number of molecules per unit volume.

Question. Which of the following statements is not correct for gas molecules?
a. Mean free path is inversely proportional to the square of diameter of gas molecules
b. Mean free path is inversely proportional to the molecular density of gas molecules
c. Mean free path is directly proportional to the pressure of gas
d. Mean free path is directly proportional to the temperature of gas
Answer : C

Question. The mean free path for air molecules at NTP is:
a. 1 Å
b. 10 Å
c. 100 Å
d. 1 mm
Answer : C

Question. Mean free path between molecules in a solid is of the order of:
a. 1 Å
b. 10 Å
c. 100 Å
d. 1 mm
Answer : A

Match the Column

Question. No gas perfect gas. Thus a real gas does not obey gas equation. It obeys van der Waal’s equation (P + a/V2) (V –b) = RT where a and b are constants. Behaviour of gas is assessed from the fact the under what conditions can it be liquefied. Gaseous state of matter is taken as gas if it cannot be liquefied by the application of pressure alone. For gas to behave as an ideal gas it has some variable  mentioned in column I. The values of these constant is mentioned in column II. Match the proper values of these constants for a gas.

Column IColumn II
(A) Critical temperature (TC) is the temperature above which gas cannot be liquefied and below which a gas can be liquefied with application of pressure alone1. 8a/27Rb
(B) Critical volume is volume of one mole of gas at critical temperature and critical pressure2. a/27b2
(C) Critical pressure is the pressure above which it can be liquefied when at initial temperature3. 3b

a. A → 1; B → 2; C → 3
b. A → 3; B → 2; C → 1
c. A → 2; B → 1; C → 3
d. A → 1; B → 3; C → 2
Answer : D

Question. Degree of freedom of a molecule is the number of coordinates to be fixed to locate the position of a molecule. The degree of freedom helps us to know the energy possessed by a molecule in real gas at given absolute temperature because, according to law of ‘Equipartition of energy’. Energy is equally divided among all degrees of freedom. For different gas the mentioned in column I, the no. of degrees of freedom per molecule is:
      Column I                Column II
(A) Monoatomic gas     1. Always 3
(B) Diatomic gas           2. Always 5
(C) Poly atomic gas      3. 4
(D) Water                      4. 7
a. A → 1; B → 2; C → 3; D → 4
b. A → 4; B → 3; C → 2; D → 1
c. A → 3; B → 4; C → 1; D → 2
d. A → 2; B → 3; C → 4; D → 1
Answer : A

Integer

Question. Two identical cylinders contain helium at 3.5 atmosphere and argon at 2.5 atmosphere respectively. If both these gases are filled in one of the cylinder, what would be the pressure of the mixture?
Answer : 6

Question. From the relation PV = RT calculate the value of the constant R for one gram mole of an ideal gas.
Answer : 2

Question. A surface is hit elastically and normally by n balls per second, each of mass m moving with velocity u. If each ball is made to hit the same surface with velocity 2u, the force on the surface would become K times. What is the value of K?
Answer : 2

Question. The rms velocity of molecules of a gas at –73°C and 1 atmospheric pressure 100 m/s. The temp. Of the gas is increased to 527°C and pressure is doubled. The rms velocity becomes K times. What is the value of K?
Answer : 2

Question. Two gases A and B, having the same temp. T, same pressure P and same volume V are mixed. If mixture occupies a volume V and has temp. T, the pressure of the mixture will be x P, where x =?
Answer : 2

Question. Suppose ideal gas equation follows VP3 = constant. Initial temperature and volume of the gas are T and V respectively. If gas expand to 27V then its temperature will be come:
Answer : 9

PERIODIC CLASSIFICATION OF ELEMENTS
 
Each of the questions given below consists of two statements, an assertion (A) and reason (R).
Select the number corresponding to the appropriate alternative as follows
(1) If both A and R are true and R is the correct explanation of A, then mark 1
(2) If both A and R are true but R is not the correct explanation of A, then mark 2
(3) If A is true but R is false, then mark 3
(4) If both A and R are false, then mark 4
 
1. A. Chlorine has higher EA than that of fluorine.
    R. Fluorine is stronger oxidising agent than chlorine.
 
2. A. Metallic character increases on going down a group from top to bottom.
    R. Ionization energy decreases on going down a group from top to bottom.
 
3. A. Mg2+ ion is smaller in size than F.
    R. Mg2+ has less number of electrons than F.
 
4. A. All the elements belonging to d-block are metals.
    R. Additional electrons are repelled more effectively by 3p electorns in Cl atom than by 2p electrons in F atom.
 
5. A. Beryllium has greater IE than boron.
    R. Boron has higher EA than beryllium.
 
6. A. Third IE of magnesium is greater than of aluminium.
    R. Mg2+ ion has stable noble gas configuration.
 
 
ANSWERS
 
PERIODIC CLASSIFICATION OF ELEMENTS
 
1. (2)
2. (1)
3. (3)
4. (3)
5. (2)
6. (1)
 
CHEMICAL BONDING
 
1. A. The melting point of LiCl is lower than that of NaCl.
    R. LiCl has predominantly covalent character whereas NaCl is predominantly ionic.
 
2. A. Pressing of two ice cube over each other cause their unificatin.
    R. Convalent bonds are formed between the water molecules at the interface.
 
3. A. XeF2 is a linear molecule.
    R. Xe atom assu,pes sp hybrid state in XeF2.
 
4. A. The bond angle of directed bonds arount S in H2S is 92º.
    R. Resonating forms go on changing into one another rapidly due to change in electronic arrangment.
 
5. A. O2 molecules in paramagnetic in nature.
    R. O2 molecule contains two unpaired electrons in pi antibonding orbitals.
 
6. A. All carbon-carbon bonds in benzene molecule are equally strong.
    R. Benzene molecule is resonance stabilised.
 
7. A. In F2C = C = CF2, the central atom is sphybridised.
    R. The F atoms on carbon 1 and 3 in F2C = C = CF2 lie on perpendicular planes.
 
8. A. A molecule with formula MX3 may or many not have trigonal planar geometry.
    R. Geometry of MX3 depends upon the number of lone pair and bond pairs around M.
 
9. A. Chlorate ion is pyramidal in shape.
    R. Hybrid state of chlorine in chlorate ion is sp3.
 
NEET Chemistry Gaseous State MCQs Set E
 
ANSWERS
 
CHEMICAL BONDING
 
1. (1)
2. (3)
3. (3)
4. (2)
5. (1)
6. (2)
7. (2)
8. (1)
9. (1)
10. (1)
 
STATES OF MATTER (GASES)
 
1. A. The product of pressure and volume for afixed amount of gas is equal to a constant represented by RT.
    R. At constant temperature, for a fixed amount of a gas, pressure is inversely proportional to volume.
 
2. A. The mixture of ideal gases A and B on their liquefaction gives ideal solution of A and B.
    R. The ideal gases cannot be liquefied.
 
3. A. The value of van der Waal constant b is higher for N2 than for NH3.
    R. NH3 molecules are associated with H–bonds.
 
4. A. At a particular temperature , the value of mean free path increases with decreases in pressure.
    R. All the gas molecules at a particular temperature possess same speed.
 
5. A. The abrupt expansion of the compressed gas always causes heating effect.
    R. The expansion causes release of energy by the gaseous system.
 
6. A. Compressibility factor of ideal gas is zero.
    R. The molecules of ideal gas are volumeless points.
 
7. A. Dry air is heavier than moist air.
    R. The vapour density of moist air lies between 9 and 14.4.
 
8. A. Rate of diffusion of N2 is more than that of CO2.
    R. Both N2 and CO2 have same value of van der Waal constant b.
 
9. A. Heat capacity of a diatomic gas is higher than that of monoatomic gas.
    R. Monoatomic gases are non-polar in nature.
 
10. A. Noble gases can be liquified.
      R. Attractive forces can exist between nonpolar molecules.
 
11. A. Noble gases have highest ionization energies in their respective periods.
      R. Noble gas have stable electronic configuration.
 
12. A. The mixture of ideal gases A and B on their liquefaction gives ideal solution of A and B.
      R. The ideal gases cannot be liquefied.
 
13. A. The value of van der Waal constant b is higher for N2 than for NH3.
      R. NH3 molecules are associated with H–bonds.
 
14. A. At a particular temperature , the value of mean free path increases with decreases in pressure.
      R. All the gas molecules at a particular temperature possess same speed.
 
15. A. Rate of diffusion of N2 is more than that of CO2.
      R. Both N2 and CO2 have same value of van der Waal constant b.
 
16. A. Noble gases can be liquified.
      R. Attractive forces can exist between nonpolar molecules.
 
 
ANSWERS
 
STATES OF MATTER (GASES)
 
1. (4)
2. (4)
3. (2)
4. (3)
5. (4)
6. (3)
7. (3)
8. (4)
9. (2)
10. (1)
11. (1)
12. (4)
13. (2)
14. (3)
15. (4)
16. (1)
Chemistry in Everyday Life
NEET UG Chemistry in Everyday Life MCQs

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