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In: Chemistry

Decide which of the following statements are true and which are false, concerning the kinetic molecular...

Decide which of the following statements are true and which are false, concerning the kinetic molecular theory.

1. The particles are assumed to exert no forces on each other; they are assumed neither to attract nor to repel each other.

2. The molecules in a real gas have finite volumes and do exert forces on each other, thus real gases do not conform to some of the assumptions of an ideal gas as stated by the kinetic molecular theory.

3. The average kinetic energy of a collection of gas particles is assumed to be inversely proportional to the Kelvin temperature of the gas.

4. The particles are in constant motion.

5. The collisions of the particles with the walls of the container are the cause of the pressure exerted by the gas.

6. The particles are so small compared with the distances between them that the volume of the individual particles can be assumed to be zero.

Solutions

Expert Solution

1)TRUE

EXPLANATION: According to kinetic theory of gases except during collisions , the interaction between the molecules are zero (negligible)

2)TRUE

EXPLANATION: By kinetic theory the volume of individual gas particles are assumed to be zero, but for real life there is no molecule with zero volume

3)TRUE

EXPLANATION: The average kinetic energy of gas particles depends on its temperature by equation

above equation valid for monoatomic gaes only

4)True

EXPLANATION: These GAS molecules are in constant, random, and rapid motion

5)TRUE

EXPLANATION: Due to collision particles have large kinetic energy , then after collision with wall of container kinetic energy converted into pressure energy

6)TRUE

All particles have compared volume , but individual particles have negligible volume

queen_honey_blossom answered 1 year ago
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