Gaseous State Test

Result

Gaseous State Test - 14

Score
-
out of -
Rank
-
out of -

TIME Taken - -

SHARING IS CARING

If our Website helped you a little, then kindly spread our voice using Social Networks. Spread our word to your readers, friends, teachers, students & all those close ones who deserve to know what you know now.

Weekly Quiz Competition

Question 1
4 / -1

At which of the following temperature would the molecules of a gas have twice the average kinetic energy they have at 20°C?

A
40°C

B
80°C

C
313°C

D
586°C

Solution
Question 2
4 / -1

A vessel contains a mixture of one mole of oxygen and two moles of nitrogen at 300 K. The ratio of the average rotational kinetic energy per O₂ molecule to that per N₂ molecule is:

A
1 : 1

B
1 : 2

C
2 : 1

D
Depends on the moments of inertia of the two molecules

Solution

Kinetic energy per degree of freedom = 1/2 kT

As diatomic gas possess two degree of freedom for rotational motion therefore rotational K.E.

In the problem both gases (oxygen and nitrogen) are diatomic and have same temperature (300 K) therefore ratio of average rotational kinetic energy will be equal to one.
Question 3
4 / -1

The average translational energy and the rms speed of molecules in a sample of oxygen gas at 300K are 6.12×10^–21J and 484m/s respectively. The corresponding values at 600K are nearly: (assuming ideal gas behaviour)

A

B

C

D

Solution

if temperature becomes twice then energy will becomes two time
Question 4
4 / -1

The temperature at which RMS velocity of SO₂ molecules is half that of He molecules at 300K is:

A
150 K

B
600 K

C
900 K

D
1200 K

Solution
Question 5
4 / -1

The rms speed of N₂ molecules in a gas is u. If the temperature is doubled and the nitrogen molecules dissociate into nitrogen atoms, the rms speed becomes:

A
u/2

B
2u

C
4u

D
14u

Solution
Question 6
4 / -1

A gas at 27°C has a volume V and pressure P. On heating its pressure is doubled and volume becomes three times. The resulting temperature of the gas will be:

A
1800°C

B
162°C

C
1527°C

D
600°C

Solution

From ideal gas equation PV = µRT we get
Question 7
4 / -1

A flask is filled with 13 gm of an ideal gas at 27°C and its temperature is raised to 52°C. The mass of the gas that has to be released to maintain the temperature of the gas in the flask at 52°C and the pressure remaining the same is:

A
2.5 g

B
2.0 g

C
1.5 g

D
1.0 g

Solution

PV ∝ Mass of gas × Temperature
Question 8
4 / -1

If the value of molar gas constant is 8.3 J/mole-K, the n specific gas constant for hydrogen in J/mole-K will be:

A
4.15

B
8.3

C
16.6

D
None of these

Solution

Specific gas constant
Question 9
4 / -1

At constant temperature on increasing the pressure of a gas by 5% will decrease its volume by:

A
5%

B
5.26%

C
4.26%

D
4.76%

Solution
Question 10
4 / -1

On 0°C pressure measured by barometer is 760 mm. What will be pressure on 100°C?

A
760 mm

B
730 mm

C
780 mm

D
None of these

Solution

From Gay Lussac’s law