To determine the number of moles of oxygen in the cylinder, we can use the ideal gas law:
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, we need to convert the pressure from mmHg to atm and the temperature from Celsius to Kelvin:
1201 mmHg = 1201 mmHg * (1 atm / 760 mmHg) = 1.58 atm
10 C = 10 + 273.15 = 283.15 K
Now we can plug in the values into the ideal gas law equation:
(1.58 atm)(2.5 L) = n(0.0821 L.atm/mol.K)(283.15 K)
3.95 = 23.26865n
n ≈ 0.170 moles
Therefore, there are approximately 0.170 moles of oxygen in the 2.5 L cylinder.
How many moles of oxygen (O2) are contained in a 2.5 L cylinder that has a pressure of 1201. mmHg and a temperature of 10. C? Be sure your answer has
the correct number of significant figures.
Note: Reference the Fundamental constants and Conversion factors for non-SI units tables for additional information.
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