Consider a 1.0 L container of Neon gas at STP. Will the average kinetic energy, average velocity,and frequency of the collisions of gas molecules with the walls of the container increase, decrease, or remain the same under each of the following conditions? a. The temperature is increased to 100 Celcius.
b. The temperature is decreased to -50 Celcius.
c. The volume is decreased to 0.50 L
d. The number of moles of neon are doubled.
a. T goes up. E goes up.
b. T goes down .....
c. V goes down so P goes up which means more collisions.
d. More mols Ne means higher P so .....
a. When the temperature is increased to 100 degrees Celsius, the average kinetic energy, average velocity, and frequency of the collisions of gas molecules with the walls of the container will all increase. According to the kinetic theory of gases, the average kinetic energy of gas molecules is directly proportional to the temperature. As the temperature increases, the gas molecules gain more energy and move faster, resulting in an increase in their average velocity. This increase in velocity leads to a higher frequency of collisions with the walls of the container.
b. When the temperature is decreased to -50 degrees Celsius, the average kinetic energy, average velocity, and frequency of the collisions of gas molecules with the walls of the container will all decrease. As the temperature decreases, the gas molecules lose energy and move slower, leading to a decrease in their average velocity. This decrease in velocity results in a lower frequency of collisions with the walls of the container.
c. When the volume is decreased to 0.50 L, the average kinetic energy, average velocity, and frequency of the collisions of gas molecules with the walls of the container will all remain the same. According to Boyle's Law, the pressure of a gas is inversely proportional to its volume, assuming constant temperature and number of moles. When the volume of the container is decreased, the gas molecules occupy a smaller space, leading to a higher frequency of collisions with the walls. However, as the volume decreases, the pressure increases proportionally, and the average velocity of gas molecules also increases. These two opposite effects cancel each other out, resulting in no net change in the average kinetic energy, average velocity, or frequency of collisions.
d. When the number of moles of neon is doubled, the average kinetic energy, average velocity, and frequency of the collisions of gas molecules with the walls of the container will all remain the same. The number of moles of a gas is directly proportional to its volume, assuming constant temperature and pressure (Avogadro's Law). When the number of moles is doubled, the volume of the gas also doubles. Since there is no change in temperature or pressure, the average kinetic energy, average velocity, and frequency of collisions remain unchanged.
To determine the changes in average kinetic energy, average velocity, and frequency of collisions of gas molecules with the walls of the container, we need to understand how each factor is affected by the given conditions. Let's go through each condition and analyze its impact:
a. The temperature is increased to 100 degrees Celsius.
When the temperature increases, the average kinetic energy and average velocity of gas molecules increase. This is because temperature is directly proportional to the average kinetic energy of gas molecules according to the kinetic theory of gases. Therefore, the average velocity and frequency of collisions with the walls of the container will also increase.
b. The temperature is decreased to -50 degrees Celsius.
When the temperature decreases, the average kinetic energy and average velocity of gas molecules decrease. Again, this is due to the relationship between temperature and average kinetic energy. Consequently, the average velocity and frequency of collisions with the walls of the container will also decrease.
c. The volume is decreased to 0.50 L.
When the volume of the container decreases, the gas molecules become more confined, resulting in an increase in the frequency of collisions with the walls. However, the average kinetic energy and average velocity remain the same since the temperature remains constant. Therefore, only the frequency of collisions increases while the average velocity remains unchanged.
d. The number of moles of neon is doubled.
Increasing the number of moles of gas molecules means there are more particles in the container. This change does not directly affect the average kinetic energy or average velocity since those depend on temperature. However, the frequency of collisions with the walls of the container increases because there are more gas molecules present.
In summary:
a. The average kinetic energy, average velocity, and frequency of collisions all increase.
b. The average kinetic energy, average velocity, and frequency of collisions all decrease.
c. The average kinetic energy and average velocity remain the same, but the frequency of collisions increases.
d. The average kinetic energy and average velocity remain the same, but the frequency of collisions increases due to an increase in the number of gas molecules.