Two equal volume containers are filled with different monatomic ideal gasses at

Question

Two equal volume containers are filled with different monatomic ideal gasses at the same temperature and pressure. One is filled with helium and the other is filled with argon (helium has a lower mass per atom than argon). Which container has the greater number of atoms? Which container has the greater internal energy? Which gas molecules are (on average) moving the fastest? If the temperature of the helium gas is increased and gas is allowed to escape so as to bring the pressure back to what it was before, how will the internal energy of the gas in the container compare to what it was before? internal energy will increase internal energy will decrease internal energy will remain the same Now Suppose a third equal volume container is filled with hydrogen gas (diatomic) at the same temperature and pressure as the argon container. Which container has the greater number of molecules? Which container has the greater Internal energy?

Explanation / Answer

We can only answer 4 questions (including subquestions) at a time . Hope this helps my friend

1) Since PV=nRT

They have the same P, V and T this means they have the same amount of moles, and since the amount of atoms in a mol is constant they have the same amount of atoms

2)

E=1.5nRT since they have the same amount of moles and Temperature they have the same Internal energy

3)

At the same temperature, the average value of the translational kinetic energy [(1/2) m <v2>] will be the same for both helium and argon. Argon has a larger mass so it will have a smaller value of <v2> or vrms. Helium has a smaller mass so it will have a larger value of <v2> or vrms

5)

They have the same P, V and T this means they have the same amount of moles, and since the amount of atoms in a mol is constant they have the same amount of atoms

E=2.5nRT the monoatomic gas has a highest internal energy

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