Question # 1

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 temperature of a gas is directly proportional to its

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average translational kinetic energy

enthalpy

internal energy

hydration energy

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

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 density of neon will be highest at

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STP

0°C, 2 atm

273°C, 1 atm

273°C, 2 atm

Density of a gas increases by

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increasing value of R

decreasing value of R

increasing T

decreasing T

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 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 pressure exerted by gas molecules is due to their

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collisions

densities

masses

kinetic energy

.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 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 motion imparted to the gas molecules by gravity is

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very small

very large

negligible

appreciable

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

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Size of

Space between

Molecular weight

both a and b

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

According to kinetic theory of gases kinetic energy depends on

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Temperature

Collision

Pressure

Atomic number

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

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 actual volume of gas molecules is considered negligible at following pressures

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2atm

4atm

6 atm

8 atm

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

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

Charles's law is only obeyed at which temperature scale

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Celsius

Kelvin

Fahrenheit

both A&B

The mono atomic gases are

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Halogens

Noble gases

6h group elements

Nitrogen and oxygen

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)

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

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

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