Question # 1

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

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

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 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

Density of a gas increases by

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increasing value of R

decreasing value of R

increasing T

decreasing T

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

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

Charles's law is only obeyed at which temperature scale

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Celsius

Kelvin

Fahrenheit

both A&B

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 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

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 motion imparted to the gas molecules by gravity is

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very small

very large

negligible

appreciable

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

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

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 relationship between density and molar mass of a gas is

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Directly proportional

^{Inversly proportional}

Straight line

Stoichiometric

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 one of the following statements is wrong for gases?

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gases do not have a definite shape and volume

volume of the gas is equal to volume of container confining the gas

confirmed gas exerts uniform pressure on the walls of its container in which it is enclosed

mass of gas cannot be determined by weighing a container in which it is enclosed

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 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 temperature of a gas is directly proportional to its

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average translational kinetic energy

enthalpy

internal energy

hydration energy

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)

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

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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