Question # 1

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)

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

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1

0.1

10

0.01

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

The pressure exerted by gas molecules is due to their

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collisions

densities

masses

kinetic energy

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 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

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

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2atm

4atm

6 atm

8 atm

The motion imparted to the gas molecules by gravity is

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very small

very large

negligible

appreciable

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 volume of a real gas

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is constant

increases with T decrease

becomes zero at absolute zero

never becomes zero

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 root mean square velocity of a gas is doubled when the temperature is

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reduced to half.

reduced to one-fourth

increased four times

inereased two times

The relationship between density and molar mass of a gas is

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Directly proportional

^{Inversly proportional}

Straight line

Stoichiometric

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

If increase in temperature and volume of an ideal gas is two times, then the initial pressure P changes to

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4P

P

2P

3P

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

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

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 temperature of a gas is directly proportional to its

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average translational kinetic energy

enthalpy

internal energy

hydration energy

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

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 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

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

Charles's law is only obeyed at which temperature scale

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Celsius

Kelvin

Fahrenheit

both A&B

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