Question # 1

Under which condition CO has the maximum molar volume.

Choose an answer

high T and P

Low T and High p

high T and low pressure

Low T and low P

The pressure exerted by gas molecules is due to their

Choose an answer

collisions

densities

masses

kinetic energy

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

Choose an answer

reduced to half.

reduced to one-fourth

increased four times

inereased two times

If volume of an ideal gas at 0C° 536cm3, what is volume at 1°C

Choose an answer

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

Choose an answer

Boyle's law

Charles's law

Graham's law

Dalton's law

Which of the statement is applicable for both ideal and real gases molecules?

Choose an answer

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

Acording to the kinetic theory of gases

Choose an answer

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

The volume of a real gas

Choose an answer

is constant

increases with T decrease

becomes zero at absolute zero

never becomes zero

At higher temperature what is true for gases

Choose an answer

pressure is decreased

volume is decreased

number of moles are decreased

KE is increased

According to kinetic theory of gases kinetic energy depends on

Choose an answer

Temperature

Collision

Pressure

Atomic number

The motion imparted to the gas molecules by gravity is

Choose an answer

very small

very large

negligible

appreciable

The molecular speed Crms of gas is

Choose an answer

Independent of temperature

Proportional to the absolute temperature

Proportional to the square root of absolute temperature

Proportional to the square of absolute temperature

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

Choose an answer

Size of

Space between

Molecular weight

both a and b

If volume of an ideal gas at 0°C 536cm3, what is volume at 1°C

Choose an answer

373 cm3

646 cm3

Becomes 0cm3

746 cm3

The density of neon will be highest at

Choose an answer

STP

0°C, 2 atm

273°C, 1 atm

273°C, 2 atm

Which of the following is the correct equation to calculate relative molecular mass of a gas

Choose an answer

M=mPRTV

M=mPR/VT

M=PV/mRT

M=mRT/PV

What are the conditions under which the relation between volume (V) and number of moles (n) of gas is plotted? (Pressure; T-temperature)

Choose an answer

constant P and T

constant P and V

constant T and V

constant n and v

Helium atom is two times heavier than a hydrogen molecule. At 298 K, the average kinetic energy of a helium atom is

Choose an answer

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

The relationship between density and molar mass of a gas is

Choose an answer

Directly proportional

^{Inversly proportional}

Straight line

Stoichiometric

According to the general gas equation, density of an ideal gas depends upon

Choose an answer

Pressure

Temperature

Molar mass of the gas

All of the above

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

Choose an answer

2 atm

1.6 atm

5 atm

I atm

More Classes

Other Links

MDCAT Chemistry Chapter 3 Gases Online Test MCQs With Answers

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer

Choose an answer