A sealed flask containing 1.0 mole of H2(g) and a sealed flask containing 2.0
moles of He(g) are at the same temperature. The two gases must have equal
1. masses
2. volumes
3. average kinetic energies
4. numbers of molecules
5 answers
I believe it is 4.
You haven't said anything about the volume of the containers or their pressures; therefore, I don't see how either 1 or 2 can be correct. The number of molecules certainly isn't correct since 2 moles He will contain twice as many molecules as 1 mole of H2.
the answer is 3
im just here for test answers lol
The answer is 3, average Kinetic energy.
The mass and volume are not given so they aren't relevant. The molarity, or concentration per liter, of the substances in flasks 1 and 2 are different, meaning they have a different number of molecules. Kinetic energy is the energy of motion and goes hand in hand with temperature. Higher temperatures=more kinetic energy/motion, and lower temperatures=less kinetic energy/motion.
The mass and volume are not given so they aren't relevant. The molarity, or concentration per liter, of the substances in flasks 1 and 2 are different, meaning they have a different number of molecules. Kinetic energy is the energy of motion and goes hand in hand with temperature. Higher temperatures=more kinetic energy/motion, and lower temperatures=less kinetic energy/motion.
3 answers