i need help on this question:
Equal masses of gaseous N2 and Ar are placed in separate flasks of equal volume at the same temperature. Tell whether each of the following statements is true or false.
a) There are more molecules of N2 are present than atoms of Ar.
true or false. how do i know which has more?
Why not take some number (any number you want to use, say 40 g). Calculate moles N2 and moles Ar.
moles N2 = 40/28 = about 1.4 so that x2 x 6.02E23 will be the # atoms N present.
moles Ar = 40/39.9 = 1.002 and that x 6.02E23 will be the # atoms Ar.
Which is larger?
To determine whether there are more molecules of N2 present than atoms of Ar, we need to compare the number of molecules of each gas.
To do this, we can use Avogadro's Law, which states that equal volumes of gases at the same temperature and pressure contain an equal number of molecules. Therefore, if the flasks have equal volumes and the gases are at the same temperature, the number of molecules of each gas will be proportional to the number of moles of each gas.
Since the masses of N2 and Ar are equal in this case, it implies that the number of moles of the two gases is also equal.
Now, let's consider the molecular formula of each gas:
- N2 is a diatomic gas, meaning it consists of two nitrogen (N) atoms bonded together. Therefore, one molecule of N2 contains 2 atoms.
- Ar is a noble gas, and it consists of single, unreactive atoms, meaning one molecule of Ar only contains 1 atom.
The fact that N2 molecules contain 2 atoms, whereas Ar molecules contain only 1 atom, means that even if the number of moles is the same, the total number of atoms will differ. Therefore, the statement "There are more molecules of N2 present than atoms of Ar" is true.