Question

Apply the kinetic molecular theory to predict the outcome regarding the gas shown at right under each of the conditions below by filling in “increases” or “decreases” in the space provided. 1. If temperature is increased, the number of collisions per second . 2. If volume is increased, the number of collisions per second . 3. If the number of particles is increased, the number of collisions per second .

Answer 1

Answer: The correct answer for

1) Increases

2) Decreases

3) Increases

Explanation: Kinetic molecular theory explained about the behavior of the gas particles.

1) The number of collisions of the particles is directly proportional to the temperature because as the temperature increases, the kinetic energy of the particles increases and therefore, the number of collisions will increase.

2) The volume is increased, the number of collisions per second will decrease because as the volume increases, the distance between the particles will increases and hence, the collisions between them will decrease.

3) The number of particles is increased, the number of collisions per second will increase because the distance between the particles will decrease and hence, the collisions between them will increase.

Answer 2

If the temperature is increased, the number of collisions per second increases.

If the volume is increased, the number of collisions per second decreases.

If the number of particles is increased, the number of collisions per second increases.

Kinetic molecular theory of gases predicts the nature of gases to be in constant motion. The theory has made conclusions about the elastic nature of gas molecules.

• The theory states that the number of collisions of the gas particles has been dependent on the temperature. With the increase in the temperature, there has been an increase in the kinetic energy of the gas molecules, which results in increased collisions. Thus, if the temperature is increased, the number of collisions per second increases.

• According to the kinetic theory, the increase in the volume of gas results in the particles moving away from each other, thereby the rate of collisions has been decreased. Thus, the increase in volume results in a decrease in the collisions per second.

• The increase in the number of particles of gas will result in more molecules being present in a small area. Thereby the collisions with the molecules will be increased. Thus, the increase in the number of particles will increase the number of collisions per second.

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