Question # 1

The mono atomic gases are

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Halogens

Noble gases

6h group elements

Nitrogen and oxygen

If volume of an ideal gas at 0°C 536cm3, what is volume at 1°C

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373 cm3

646 cm3

Becomes 0cm3

746 cm3

.The number of moles in 2.24 dm3 of H2 gas at STP is:

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1

0.1

10

0.01

Which one of the following statements is wrong for gases?

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gases do not have a definite shape and volume

volume of the gas is equal to volume of container confining the gas

confirmed gas exerts uniform pressure on the walls of its container in which it is enclosed

mass of gas cannot be determined by weighing a container in which it is enclosed

For an ideal gas, number of mole in terms of its pressure P, temperature T and gas constant is

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PT/R

PRT

PV/RT

RT/P

According to the general gas equation, density of an ideal gas depends upon

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Pressure

Temperature

Molar mass of the gas

All of the above

The volume of a real gas

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is constant

increases with T decrease

becomes zero at absolute zero

never becomes zero

Acording to the kinetic theory of gases

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The pressure exerted by a gas is proportional to mean square velocity of the molecules

The pressure exerted by the gas is proportional to the root mean square velocity of the molecules

The root mean square velocity is inversely proportional to the temperature

The mean translational KE of the molecule is directly proportional to the absolute temperature

At higher temperature isotherm of Boyle's law moves away from both axis, is due to increase in

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pressure

No. of moles

Volume

all of these

The volume of given mass of gas is directly proportional to absolute temperature when pressure is kept constant this is called

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Boyle's law

Charles's law

Graham's law

Dalton's law

Which of the statement is applicable for both ideal and real gases molecules?

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Have no forces of attraction

Collisions between the molecules is elastic

Molecules are in random movement

The actual volume of gas is negligible as compared to the volume of gas

Under which condition CO has the maximum molar volume.

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high T and P

Low T and High p

high T and low pressure

Low T and low P

The actual volume of gas molecules is considered negligible at following pressures

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2atm

4atm

6 atm

8 atm

An ideal gas, obeying Kinetic theory of gases cannot be liquified, because

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its critical temperature is above 0°C

its molecules are relatively small in size

It solidifies before becoming a liquid

Forces acting between its molecules are negligible

Which of the following is the correct equation to calculate relative molecular mass of a gas

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M=mPRTV

M=mPR/VT

M=PV/mRT

M=mRT/PV

The number of molecules in 22.4 dm3 of gas at 0°C and 1 atm are

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6.02×10(23)

6.02× 10(25)

6.02×10(22)

6.02×10(21)

One dm3 of H2 and O2: has different masses but no. of particles are

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same

H2 has greater

different

O2 has greater

If a gas expands at constant temperature

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The pressure decreases

The Kinetic energy of the molecules remains the same

The kinetic energy of the molecules decreases

The number of molecules of the gas increase

At higher temperature isotherm of Boyle's law moves away from both axis, is due to increase in:

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pressure

No. of moles

Volume

All

Helium atom is two times heavier than a hydrogen molecule. At 298 K, the average kinetic energy of a helium atom is

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same as that of a hydrogen molecule

half that of a hydrogen molecule

two times that of a hydrogen molecule

four times that of hydrogen molecule

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