CHEM 1B Lecture 3: Chem 1B Smith lecture notes 3

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carmineprairie-dog920

21 Jan 2018

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Average kinetic energy of gas molecules decreases with decreasing temp; as well as average speed. All the gas molecules in the sample cannot have the same kinetic energy. There are gas molecules that move slower than average. 1 liter of h2 liters nh3. Gas is modeled as a collection of small particles in a large volume with lots of empty space between the particles. Particles are constantly moving in random directions and with different speed. Particles undergo elastic collisions and exchange energy; there is no overall loss of kinetic energy. Temperature is defined as a measure of the average kinetic energy of particles. Root mean square speed ( m = molecular weight) Example: calculate the root mean square velocity of oxygen molecules of 25 c. Molecules do not have the same speed; molecular speed distribution can be measured experimentally. The speed distribution spreads out as temperature gets higher.

Related Questions

Explain in molecular terms why the pressure of a gas increases with increasing temperature when the volume is held constant.

	As the temperature increases, kinetic energy of gas particles increases which in turn decreases both the average force of collisions and the frequency of collisions.
	As the temperature increases, kinetic energy of gas particles decreases which in turn decreases both the average force of collisions and the frequency of collisions.
	As the temperature increases, kinetic energy of gas particles decreases which in turn increases both the average force of collisions and the frequency of collisions.
	As the temperature increases, kinetic energy of gas particles increases which in turn increases both the average force of collisions and the frequency of collisions.