Question

This problem will review one of the questions in the ideal gas, but with numbers:

You have one container of hydrogen, and another container of oxygen. The number of molecules, temperature and volume are the same for both gases. Oxygen is, however, heavier than hydrogen.  

How does the average kinetic energy of hydrogen compare to oxygen?

Hydrogen has LARGER average kinetic energy than oxygen.

Hydrogen has THE SAME average kinetic energy as oxygen.

Hydrogen has LESS average kinetic energy than oxygen.

How does the average velocity of hydrogen compare to the average velocity of oxygen?

Hydrogen is moving FASTER than oxygen

Hydrogen is moving at the SAME speed as oxygen.

Hydrogen is moving SLOWER than oxygen.

In lab, we noted that pressure (which should be the same for both gases) is a product of the strength of the collision times the frequency of collisions. The strength is proportional to mv, and the frequency is proportional to v.

If we take the mass of hydrogen to be 4 kg and the speed to be 3 m/s (yes - these numbers are ridiculous for a molecule of gas - but the goal here is to focus on concepts and not get realistic numbers), and if we take the mass of oxygen to be 9kg, what is the speed of the oxygen?

speed of oxygen =	nothing	m/s

What is the strength (mv) for the hydrogen?

strength of hydrogen collision =	nothing	kg m/s

Which statement summarizes how hydrogen (a less massive element) can exert the same pressure as oxygen (a more massive element) at the same temperature, volume, and number of molecules?

Hydrogen collisions with the walls are more frequent but less strong compared to oxygen.

Hydrogen collisions with the walls are equally frequent and equally strong compared to oxygen.

Hydrogen collisions with the walls are less frequent but more strong compared to oxygen.

Answer 1