# If 300 ml of a gas at 27°C is cooled to 7°C at constant pressure, its final volume will be: 1. 135 ml 2. 540 ml 3. 350 ml 4. 280 ml

Subtopic:  Gas Laws |
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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-

($R=0.0821$ $L$ $atm$ ${K}^{-1}$ $mol{e}^{-1}$)

1. 3.90 atm

2. 4.92 atm

3. 6.02 atm

4. 2.96 atm

Subtopic:  Ideal Gas Law |
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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. 1 atm

2. 4 atm

3. 3 atm

4. 2 atm

Subtopic:  Ideal Gas Law |
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The density of methane at 2.0 atmosphere pressure and 27°C is-

1. 0.13 gL–1

2. 0.26 gL–1

3. 1.30 gL–1

4. 2.60 gL–1

Subtopic:  Gas Laws |
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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 ${27}^{o}C$. If the total pressure exerted by these non-reacting gases is one atmosphere, the partial pressure exerted by nitrogen is-

1. 1 atm

2. 0.1 atm

3. 0.2 atm

4. 0.4 atm

Subtopic:  Dalton's Law |
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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-

1. 180 mm

2. 360 mm

3. 540 mm

4. 720 mm

Subtopic:  Dalton's Law |
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Maximum deviation from ideal gas is shown by-

1. H2(g)

2. N2(g)

3. CH4(g)

4. NH3(g)

Subtopic:  Liquefaction of Gases & Liquid |
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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. 1.0 J

2. 4.15 J

3. 2493 J

4. 3.3 J

Subtopic:  Kinetic Theory of Gas |
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1.6 g O2 gas and 0.1 g H2 gas are placed in a 1.12 L flask at 0 oC. The total pressure of the gas mixture will be-

1. 2 atm

2. 3 atm

3. 4 atm

4. 1 atm

Subtopic:  Ideal Gas Law |
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Which among the following mixtures of gases at room temperature does not obey Dalton's law of partial pressure-

1. He and O2

2. NH3 and HCl

3. H2 and He

4. N2 and He

Subtopic:  Dalton's Law |
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