# of moles of oxygen in 2 L @ 24 deg C & 750 torr?
Use PV = nRT
Remember T must be in kelvin.
kbj
To determine the number of moles of oxygen in a given volume at a specific temperature and pressure, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (in atmospheres)
V = Volume (in liters)
n = Number of moles
R = Ideal gas constant (0.0821 L.atm/mol.K)
T = Temperature (in Kelvin)
First, let's convert the given values to the appropriate units:
- 24 degrees Celsius = 24 + 273.15 = 297.15 Kelvin
- 750 torr = 750/760 atm (since 1 atm = 760 torr) = 0.987 atm
Now we can plug the values into the ideal gas law equation to find the number of moles:
(0.987 atm) * (2 L) = n * (0.0821 L.atm/mol.K) * (297.15 K)
Simplifying the equation, we can solve for n:
n = (0.987 atm * 2 L) / (0.0821 L.atm/mol.K * 297.15 K)
n ≈ 0.0845 moles
Therefore, there are approximately 0.0845 moles of oxygen in a 2-liter container at 24 degrees Celsius and 750 torr.