Question # 1

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

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

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)

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

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

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

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

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 number of moles in 2.24 dm3 of H2 gas at STP is:

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1

0.1

10

0.01

The mono atomic gases are

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Halogens

Noble gases

6h group elements

Nitrogen and oxygen

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

The temperature of a gas is directly proportional to its

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average translational kinetic energy

enthalpy

internal energy

hydration energy

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

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

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

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

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Size of

Space between

Molecular weight

both a and b

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

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

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

Charles's law is only obeyed at which temperature scale

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Celsius

Kelvin

Fahrenheit

both A&B

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