# Problem: If equal masses of O 2(g) and HBr(g) are in separate containers of equal volume and temperature, which one of the following statements is true?   a) The pressure in the O 2 container is greater than that in the HBr container. b) There are more HBr molecules than O 2 molecules. c) The average velocity of the O 2 molecules is less than that of the HBr molecules. d) The average kinetic energy of HBr molecules is greater than that of O 2 molecules. e) The pressures of both gases are the same.

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###### Problem Details

If equal masses of O 2(g) and HBr(g) are in separate containers of equal volume and temperature, which one of the following statements is true?

a) The pressure in the O 2 container is greater than that in the HBr container.

b) There are more HBr molecules than O 2 molecules.

c) The average velocity of the O 2 molecules is less than that of the HBr molecules.

d) The average kinetic energy of HBr molecules is greater than that of O 2 molecules.

e) The pressures of both gases are the same.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Kinetic Molecular Theory concept. You can view video lessons to learn Kinetic Molecular Theory. Or if you need more Kinetic Molecular Theory practice, you can also practice Kinetic Molecular Theory practice problems.

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Based on our data, we think this problem is relevant for Professor Castaneda's class at UMICH.