Question # 1

The Van der Waals' equation explain the behaviour of.

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Ideal gas

Real gas

Vapours

Non ideal gases

For a gas obeying Boyle's law if pressure is doubled, the volume becomes.

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Double

One half

Four times

Remains constant

Rate of diffusion of CO and N₂are same at room temperature due to the reason, that

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Both are diatomic molecules

Both have same multiple bond in them

Both have lone pairs in them

Both have same molar masses

What are the SI of excluded volume 'b' in Vander waal equation.

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dm³ mol -1

m3 mol -1

mol dm-3

mol m-3

Equal masses of methane and oxygen are mixed in an empty container at 25 ^oC. The fraction of total pressure exerted by oxygen is.

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1/3

8/9

1/9

16/17

The temperature of natural plasma is about.

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200000 ^oC

10000^oC

5000^oC

1000^oC

The rate of diffusion of a gas is

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Directly proportional to its density

Directly proportional to molecular mass

Inversely proportional to its density

Inversely proportional to square root of its molecular mass

Gases of air, always remains in the random motion and do not settle due to.

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Elastic collision of gas molecules

Unequal number of different gas molecules

Difference impartial pressure of gas molecules

Difference in molecular masses of air gases

If absolute temperature of gas is doubled and the pressure is reduced to one half, the volume of the gas will.

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Remain unchanged

Increase four times

Reduce to 1/4

Be doubled

Which one of the following expressions is for ideal gas equation.

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PM= nRT

PV = nRT

PV = dRT

PV= nTP

If temperature of one mole of ideal gas at 273 K and one atmospheric pressure is increased by 1 K, amount of energy absorbed is.

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0.082 dm3 atm

1.987 cal.

8.313 J

All are correct.

The volume of a gas at 0 oC is 273 dm3, the pressure remaining constant. At which temperature its volume will be doubled.

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273 K

273 ^oC

546 ^oC

316 K

Under which conditions of temperature and pressure will a real gas behave most like an ideal gas.

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Low temperature and how pressure

High temperature and high pressure

Low temperature and high pressure

High temperature and low pressure

In gas occupies a volume of 2 dm³at 27°C and I atm pressure. The expression for its volume at S.T.P. is

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Which is not example of natural plasma.

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Lightening bolt

Aurora

Neon sign

Sum

Keeping the temperature constant of the gas is expanded.

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Pressure will decrease

Temperature will increase

Kinetic energy of molecules will increase

No. of gas molecules increases

What are the SI units of Van der Waal constant 'a'

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atm dm3 mol-2

atm dm6 mol-2

Nm4 mol-2

Nm mol-1

Observed pressure is less than ideal pressure for any gas due to

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Intermolecular forces

Size of molecules

Boiling point of molecules

Both a and c

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