Question # 1

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

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

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

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Size of

Space between

Molecular weight

both a and b

The motion imparted to the gas molecules by gravity is

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very small

very large

negligible

appreciable

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

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

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 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

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

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 relationship between density and molar mass of a gas is

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Directly proportional

^{Inversly proportional}

Straight line

Stoichiometric

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

The pressure exerted by gas molecules is due to their

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collisions

densities

masses

kinetic energy

The volume of a real gas

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is constant

increases with T decrease

becomes zero at absolute zero

never becomes zero

At constant volume, for a fixed number of moles of a gas the pressure of the gas increases with size of temperature due to

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increase in average molecular speed

increase in number of moles

increase in molecular attraction

decrease in the distance between the molecules

If temperature is 73K and volume is 146 cm3 then calculate the value of K=V/T

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5

4

3

2

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

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 P

Low T and low P

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

The temperature of a gas is directly proportional to its

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average translational kinetic energy

enthalpy

internal energy

hydration energy

According to kinetic theory of gases kinetic energy depends on

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Temperature

Collision

Pressure

Atomic number

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