The volume of a gas is 100 ml at 100°C. If the pressure remains constant then the temperature at which the volume becomes 200 ml is-

  • 200°C

  • 473°C

  • 746°C

  • 50°C

If 300 ml of a gas at 27°C is cooled to 7°C at constant pressure, its final volume will be-

  • 135 ml

  • 540 ml

  • 350 ml

  • 280 ml

A flask containing air (open to atmosphere) is heated from 300 K to 500 K. The percentage of air escaped to the atmosphere is nearly- 

  • 16.6

  • 40

  • 66

  • 20

According to Charle’s law, at constant pressure, 100 ml of a given mass of a gas with 10°C rise in temperature will become 1273=0.00366 ,T initial = Zero °C

  • 100.03

  • 99.96

  • 103.66

  • 100.36

A sealed tube which can withstand a pressure of 3 atmosphere is filled with air at 27oC and 760 mm pressure. The tube will burst at - 

  • 900°C

  • 627°C

  • 726°C

  • 1173°C

The pressure of 2 moles of an ideal gas at 546 K having volume 44.8 L is

  • 2 atm

  • 3 atm

  • 4 atm

  • 1 atm

The number of moles of H2 in 0.224 litre of hydrogen gas at STP (273 K, 1 atm.) is-

  • 1

  • 0.1

  • 0.01

  • 0.001

120 g of an ideal gas of molecular weight 40 g mole–1 are confined to a volume of 20 L at 400 K. The pressure of the gas is- 

 (R=0.0821 L atm K−1 mole−1)

  • 3.90 atm

  • 4.92 atm

  • 6.02 atm

  • 2.96 atm

The volume of 2.8 g of carbon monoxide at 27°C and 0.821 atm pressure is- 

(R=0.0821 lit atm K−1 mol−1)

  • 0.3 litre

  • 1.5 litre

  • 3 litre

  • 30 litre

3.2 g of oxygen  and 0.2 g of hydrogen are placed in a 1.12 litre flask at 0°C.

The total pressure of the gas mixture will be-

  • 1 atm

  • 4 atm

  • 3 atm

  • 2 atm

The density of methane at 2.0 atmosphere pressure and 27°C is- 

  • 0.13 gL–1

  • 0.26 gL–1

  • 1.30 gL–1

  • 2.60 gL–1

The volume of 0.0168 mol of O2 obtained by decomposition of KClO3 and collected by displacement of water is 428 ml at a pressure of 754 mm Hg at 25°C. The pressure of water vapour at 25°C is- 

  • 18 mm Hg

  • 20 mm Hg

  • 22 mm Hg

  • 24 mm Hg

The partial pressure of H2 in a flask containing 2 g of H2, 14 g of N2, and 16 g of O2 is-

  • 1/2 of the total pressure

  • 1/3 of the total pressure

  • 1/4 of the total pressure

  • 1/16 of the total pressure

Equal weights of methane and oxygen are mixed in an empty container at 25°C. The fraction of the total pressure exerted by oxygen is- 

  • 1/3

  • 1/2

  • 2/3

  •  13×273298  

In a flask of volume V litres, 0.2 mol of oxygen, 0.4 mol of nitrogen, 0.1 mol of ammonia and 0.3 mol of helium are enclosed at 27oC. If the total pressure exerted by these non-reacting gases is one atmosphere, the partial pressure exerted by nitrogen is-

  • 1 atm

  • 0.1 atm

  • 0.2 atm

  • 0.4 atm

Equal weights of ethane and hydrogen are mixed in an empty container at 25°C. The fraction of the total pressure exerted by hydrogen is- 

  • 1 : 2

  • 1 : 1

  • 1 : 16

  • 15 : 16

A gaseous mixture contains 56 g of N2, 44 g of CO2 and 16 g of CH4. The total pressure of the mixture is 720 mm Hg. The partial pressure of CH4 is-

  • 180 mm

  • 360 mm

  • 540 mm

  • 720 mm

The time taken for a certain volume of a gas ‘X’ to diffuse through a small hole is 2 minutes. It takes 5.65 minutes for oxygen to diffuse under the similar conditions. The molecular weight of ‘X’ is [NCERT 1990]

  • 8

  • 4

  • 16

  • 32

The rate of diffusion of methane at a given temperature is twice that of gas X. The molecular weight of X is 

  • 64.0

  • 32.0

  • 4.0

  • 8.0

Density ratio of O2 and H2 is 16 : 1. The ratio of their r.m.s. velocities will be- 

  • 4 : 1

  • 1 : 16

  • 1 : 4

  • 16 : 1

The rate of diffusion of a gas having molecular weight just double of nitrogen gas is 56 mls–1. The rate of diffusion of nitrogen will be

  • 79.19 ml s–1

  • 112.0 ml s–1

  • 56 ml s–1

  • 90.0 ml s–1

50 ml of gas A diffuse through a membrane in the same time as 40 ml of a gas B under identical pressure-temperature conditions. If the molecular weight of A is 64, that of B would be [CBSE PMT 1992]

  • 200

  • 80

  • 100

  • 250

The kinetic energy for 14 grams of nitrogen gas at 127°C is nearly (mol. mass of nitrogen = 28 and gas constant = 8.31JK–1mol–1) 

  • (1) 0 J

  • (2) 4.15 J

  • (3) 2493 J

  • (4) 3.3 J

The rms velocity of CO2 at a temperature T (in kelvin) is x cms–1. At what temperature (in kelvin) the rms velocity of nitrous oxide would be 4x cms–1

  • 16 T

  • 2 T

  • 4 T

  • 32 T

The rms velocity of an ideal gas at 27°C is 0.3 ms–1. Its rms velocity at 927°C (in ms–1) is [IIT 1996; EAMCET 1991]

  • 3.0

  • 2.4

  • 0.9

  • 0.6

The rms velocity of hydrogen is 7times the rms velocity of nitrogen. If T is the temperature of the gas [IIT 2000]

  • T(H2)=T(N2)

  • T(H2)>T(N2)

  • T(H2)<T(N2)

  • T(H2)=7T(N2)

If the average velocity of N2 molecules is 0.3 m/s at 27°C, then the velocity of 0.6 m/s will take place at 

  • 273 K

  • 927 K

  • 1000 K

  • 1200 K

The temperature of an ideal gas is reduced from 927°C to 27°C. The rms velocity of the molecules becomes

  • Double the initial value

  • Half of the initial value

  • Four times the initial value

  • Ten times the initial value

Equal moles of hydrogen and oxygen gases are placed in container with a pin-hole through which both can escape. What fraction of the oxygen escapes in the time required for one-half of the hydrogen to escape?

  • 1/4         

  • 3/8         

  • 1/2           

  • 1/8

A gas such as carbon monoxide would be most likely to obey the ideal gas law at-

  • High temperature and low pressure

  • Low temperature and high pressure

  • High temperature and high pressure

  • Low temperature and low pressure

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