Chemistry, 12.02.2020 04:19 monsterenergy19

Check all the true statements concerning two identical containers, one with helium gas in it and one with xenon gas. Choose one or more:

a. When the temperature of either sample of gas increases, the root-mean-square speed increases.
b. If both gases are at the same temperature, they have the same average kinetic energy.
c. When the temperature of either sample of gas increases, the number of particles with average kinetic energy increases.
d. If both of the containers are at the same temperature, they will have the same root-mean-square speed.

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When the temperature of either sample of gas increases, the root-mean-square speed increases is a true statement. If both gases are at the same temperature, they have the same average kinetic energy is a true statement.When the temperature of either sample of gas increases, the number of particles with average kinetic energy increases is a true statement. If both of the containers are at the same temperature, they will have the same root-mean-square speed is a false statement.

The RMS velocity is said to be directly proportional to the square root of temperature and then inversely proportional to the square root of molar mass.

When there is an increase is temperature, the average speed and kinetic energy of the gas molecules also increase.

When comparing two gases at the same temperature, note that the molecules of the gas with the smaller molecular weight often have the higher RMS speed.

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Answer from: bella2284

The answers to the question are as follows

a. True

b. True

c. True

d. false

Explanation:

The requiredrelation is

$u_{rms} = \sqrt{\frac{3RT}{m} }$

Where R = The gas constant

T = the temperature in kelvin

m = molecular mass

$u_{rms}$ = root mean square speed

From the above relation on the kinetic energy of a gas we have the following true statements

a. When the temperature of either of the sample of gas increases, the root-mean-square speed increases.

This statement is true as the root means square velocity is directly proportional to the square root of the temperature a. is true

b. If both gases are at the same temperature, they have the same average kinetic energy.

From the equation for the average kinetic energy $KE_{avg} = \frac{3}{2} RT$ we see that the kinetic energy is directly proportional to its Kelvin temperature and hence b. is true

c. When the temperature of either sample of gas increases, the number of particles with average kinetic energy increases.

This statement is true as shown in the kinetic energy equation

d. If both of the containers are at the same temperature, they will have the same root-mean-square speed.

This statement is false as xenon and helium have different, molecular masses

Answer from: Quest

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Answer from: Quest

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