Two flasks of equal volume and at the same temperature contain different gases. one flask contains 5.0 g of o2, and the other flask contains 5.0 g of h2. is each of the following statements true or false? explain.
a) true. because the gases have the same volumes, they must have the same number of molecules.
b) false. because the molar mass of o2 is greater than the molar mass of h2, 5.0g of o2 will contain fewer molecules than 5.0 g of h2.
c)false. depending on the pressure each flask may contain different numbers of molecules.

Explanation:

This law states that volume is directly proportional to number of moles at constant temperature and pressure.

Mathematically,    

As the given gases have same volume so they will have same number of moles.

Hence, the statement gases have the same volumes, they must have the same number of molecules, is true.

 No. of moles of =

                               =

                               = 0.156 mol

Hence, no. of molecules of =

                              = molecules

No. of moles of =

                               =

                               = 2.5 mol

Hence, no. of molecules of =

                              = molecules

As, molar mass of oxygen gas is different as compared to the molar mass of hydrogen gas. Therefore, the statement 5.0 g of is not true.

                      (at constant temperature and number of moles)

Therefore, when volume of both the gases is same then pressure should also be the same.

Hence, the statement depending on the pressure each flask may contain different numbers of molecules, is false.

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