Question # 1

Which type of motion is exhibited by gases?

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Vibrational

Transitional

Rotational

All of them

Gas is enclosed in a container of 20cm3 with the moving piston. According to kinetic theory of gases, what is the effect on freely moving molecules of the gas if temperature is increased from 20°C to 100C.

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Colliding capability of molecule will become lower

Pressure will become one half

Temperature has no effect on freely moving molecules

Volume will be increased

The volume of gas depends upon the------- moleules

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Size of

Space between

Molecular weight

both a and b

According to kinetic theory of gases kinetic energy depends on

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Temperature

Collision

Pressure

Atomic number

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

The relationship between density and molar mass of a gas is

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Directly proportional

^{Inversly proportional}

Straight line

Stoichiometric

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

Theoretically, the temperature at which volume of gas become equal to zero is called

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Boiling point of water

Zero absolute

Zero Kelvin

both B and C

The temperature of a gas is directly proportional to its

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average translational kinetic energy

enthalpy

internal energy

hydration energy

The density of neon will be highest at

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STP

0°C, 2 atm

273°C, 1 atm

273°C, 2 atm

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

Which is not true in case of an ideal gas?

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It cannot be converted into a liquid

There is no interaction between the molecules

All molecules of the gas move with same speed

At a given temperature P'V is proportional to the amount of the gas

If volume of an ideal gas at 0C° 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

What are the conditions under which the relation between volume (V) and number of moles (n) of gas is plotted? (Pressure; T-temperature)

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constant P and T

constant P and V

constant T and V

constant n and v

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

The molecular speed Crms of gas is

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Independent of temperature

Proportional to the absolute temperature

Proportional to the square root of absolute temperature

Proportional to the square of absolute temperature

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

At absolute zero the molecules of hydrogen gas will have

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Only translatioral motion

Only vibrational motion

Only rotational motion

All the motion are ceased

An ideal gas expands according to PV=constant. On expansion, the temperature of gas

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will rise

will drop

cannot be determined because the exteral pressure is not known

will remain same

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