Question # 1

The pressure exerted by gas molecules is due to their

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collisions

densities

masses

kinetic energy

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

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1

0.1

10

0.01

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

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

Which type of motion is exhibited by gases?

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Vibrational

Transitional

Rotational

All of them

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 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)

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

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

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Size of

Space between

Molecular weight

both a and b

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

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

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

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

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

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 temperature of a gas is directly proportional to its

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average translational kinetic energy

enthalpy

internal energy

hydration energy

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

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

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

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