explain why a balloon with 1.00 mol xe gas in it has the same volume as balloon with 1.00 mol he gas in it
Gas molecules spread out depending on temperature an pressure, not mass. So all gases spread equally..
What is the temperature of a 1.02 mol gas sample that occupies 17.3 L at 753 torr?
To understand why a balloon with 1.00 mol of Xe gas has the same volume as a balloon with 1.00 mol of He gas, we need to consider the principles of ideal gas behavior and Avogadro's law.
Avogadro's law states that equal volumes of gases, at the same temperature and pressure, contain an equal number of particles (atoms, molecules, or formula units). This means that when comparing the same number of moles of different gases, they will occupy the same volume.
The ideal gas law equation, PV = nRT, describes the relationship between pressure (P), volume (V), moles (n), gas constant (R), and temperature (T). In this case, we can assume that the temperature and pressure are constant, so we can simplify the equation to V = nR/P.
Since the number of moles (n) is the same for both the Xe and He gases (1.00 mol), and the gas constant (R) is a fixed value, the volume (V) of the balloons will be directly proportional to each other.
Therefore, a balloon with 1.00 mol of Xe gas will have the same volume as a balloon with 1.00 mol of He gas, assuming they are at the same temperature and pressure.