Answer :
To determine which gas exerts a higher pressure, we can use the ideal gas law equation:
[tex]PV = nRT[/tex]
Where:
- [tex]P[/tex] is the pressure,
- [tex]V[/tex] is the volume,
- [tex]n[/tex] is the number of moles of the gas,
- [tex]R[/tex] is the ideal gas constant, and
- [tex]T[/tex] is the temperature.
In this question, both gases are in identical 5.0 L chambers at room temperature, so the volume ([tex]V[/tex]) and temperature ([tex]T[/tex]) can be considered as constants, and we are comparing the pressure based on the number of moles ([tex]n[/tex]) of each gas. The ideal gas constant ([tex]R[/tex]) is also a constant value, so the pressure will depend directly on the number of moles of gas present:
Calculate the number of moles for each gas:
For O₂ (oxygen):
- The molar mass of O₂ is approximately 32.00 g/mol.
- The number of moles, [tex]n[/tex], is calculated as:
[tex]n = \frac{5.00 \text{ g}}{32.00 \text{ g/mol}} = 0.15625 \text{ mol}[/tex]
For He (helium):
- The molar mass of He is approximately 4.00 g/mol.
- The number of moles, [tex]n[/tex], is calculated as:
[tex]n = \frac{5.00 \text{ g}}{4.00 \text{ g/mol}} = 1.25 \text{ mol}[/tex]
Compare the number of moles:
Helium (He) has more moles (1.25 mol) compared to oxygen (O₂) (0.15625 mol) for the same mass of gas.
Conclude the pressure comparison:
Since the number of moles is directly proportional to pressure in the ideal gas law (assuming constant temperature and volume), the chamber with helium (He) will exert a higher pressure than the chamber with oxygen (O₂).
In conclusion, the chamber containing helium (He) has the higher pressure at room temperature.