A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. c. The molecules of which gas have the greater average kinetic energy?

Verified step by step guidance

insert step 1> Understand that the average kinetic energy of gas molecules is related to temperature.

insert step 2> Recall that according to the kinetic molecular theory, the average kinetic energy of gas molecules is given by the equation: \( KE_{avg} = \frac{3}{2}kT \), where \( k \) is the Boltzmann constant and \( T \) is the temperature in Kelvin.

insert step 3> Note that the average kinetic energy of gas molecules depends only on the temperature of the gas, not on the type of gas or its molar mass.

insert step 4> Since both nitrogen and xenon are at the same temperature (room temperature), their molecules have the same average kinetic energy.

insert step 5> Conclude that the molecules of nitrogen and xenon have equal average kinetic energy at the same temperature.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Kinetic Molecular Theory

The Kinetic Molecular Theory explains the behavior of gases in terms of particles in constant motion. It states that the average kinetic energy of gas molecules is directly proportional to the temperature of the gas in Kelvin. This means that at the same temperature, all gases have the same average kinetic energy, regardless of their molecular mass.

Temperature and Kinetic Energy

Temperature is a measure of the average kinetic energy of the particles in a substance. In the context of gases, if two gases are at the same temperature, their average kinetic energies will be equal. Therefore, the average kinetic energy of nitrogen and xenon in the flask will be the same since they are both at room temperature.

Molecular Mass and Speed

While the average kinetic energy of gas molecules is the same at a given temperature, the speed of the molecules varies with their mass. Lighter molecules, like nitrogen (N2), move faster than heavier molecules, like xenon (Xe). This difference in speed does not affect the average kinetic energy but is important for understanding the behavior of gases in terms of diffusion and effusion.

Recommended video:

Guided course

00:57

Speed of Light Formula

Related Practice

Textbook Question

Carbon monoxide gas reacts with hydrogen gas to form methanol. CO(g) + 2 H₂(g) → CH₃OH(g) A 1.50-L reaction vessel, initially at 305 K, contains carbon monoxide gas at a partial pressure of 232 mmHg and hydrogen gas at a partial pressure of 397 mmHg. Identify the limiting reactant. Determine the theoretical yield of methanol in grams.

views

Textbook Question

Consider a 1.0-L sample of helium gas and a 1.0-L sample of argon gas, both at room temperature and atmospheric pressure. a. Do the atoms in the helium sample have the same average kinetic energy as the atoms in the argon sample?

views

Textbook Question

A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. a. Which of the two gases exerts the greater partial pressure?

Textbook Question

Calculate the root mean square velocity of F₂, Cl₂, and Br₂ at 298 K.

Textbook Question

Calculate the kinetic energy of F₂, Cl₂, and Br₂ at 298 K.

views

Textbook Question

Calculate the root mean square velocity and kinetic energy of F₂, Cl₂, and Br₂ at 298 K. Rank these three halogens with respect to their rate of effusion.