Lesson: Distribution of Molecular Speeds
In this lesson, we will learn how to calculate the proportion of particles, in an ideal gas, that have a given speed using the Maxwell–Boltzmann distribution function.
Sample Question Videos
Worksheet: Distribution of Molecular Speeds • 6 Questions • 2 Videos
An incandescent light bulb is filled with neon gas. The gas that is in close proximity to the element of the bulb is at a temperature of K. Determine the root-mean-square speed of neon atoms in close proximity to the element. Use a value of 20.2 g/mol for the molar mass of neon.
Helium atoms in a gas that is at a temperature have a root-mean-square speed of 196 m/s. When the gas is heated until it becomes a plasma with a temperature , the root-mean-square speed of the helium atoms is 618 km/s. Use a value of 4.003 g/mol for the molar mass of helium.
Using the approximation for small , estimate the fraction of nitrogen molecules at a temperature of K that have speeds between 290 m/s and 291 m/s. A nitrogen molecule has a mass of kg.
Find the ratio for hydrogen gas at a temperature of 77.0 K. Use a molar mass of 2.02 g/mol for hydrogen gas.
In a sample of a monatomic gas, a number of molecules have speeds that are within a very small range around the root-mean-square speed of atoms in the gas, . A number of molecules have speeds that are within the same very small range around a speed of . Determine the ratio of to .
A sample of nitrogen is at a temperature of K. has a molar mass of 28.00 g/mol.
What is the most probable speed of the nitrogen molecules?
What is the average speed of the nitrogen molecules?
What is the root-mean-square speed of the nitrogen molecules?