Question # 1

According to kinetic theory of gases kinetic energy depends on

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Temperature

Collision

Pressure

Atomic number

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 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)

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

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 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

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

At higher temperature what is true for gases

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pressure is decreased

volume is decreased

number of moles are decreased

KE is increased

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

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

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

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Size of

Space between

Molecular weight

both a and b

Which type of motion is exhibited by gases?

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Vibrational

Transitional

Rotational

All of them

The pressure exerted by gas molecules is due to their

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collisions

densities

masses

kinetic energy

Charles's law is only obeyed at which temperature scale

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Celsius

Kelvin

Fahrenheit

both A&B

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

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

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

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

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

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 a real gas

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is constant

increases with T decrease

becomes zero at absolute zero

never becomes zero

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

Density of a gas increases by

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increasing value of R

decreasing value of R

increasing T

decreasing T

The pressure of gas at constant temperature in a container of 2dm3 is 10 atm what will be its final pressure if it is connected with 10 dm3 container

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2 atm

1.6 atm

5 atm

I atm

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