Question # 1

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 mono atomic gases are

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Halogens

Noble gases

6h group elements

Nitrogen and oxygen

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

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

An ideal gas expands according to PV=constant. On expansion, the temperature of gas

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will rise

will drop

cannot be determined because the exteral pressure is not known

will remain same

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

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

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

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

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2atm

4atm

6 atm

8 atm

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 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 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

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

One dm3 of H2 and O2: has different masses but no. of particles are

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same

H2 has greater

different

O2 has greater

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

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

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

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

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 relationship between density and molar mass of a gas is

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Directly proportional

^{Inversly proportional}

Straight line

Stoichiometric

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

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Size of

Space between

Molecular weight

both a and b

The temperature of a gas is directly proportional to its

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average translational kinetic energy

enthalpy

internal energy

hydration energy

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

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