We’re going to calculate the pressure of each gas first using the ideal gas equation:
P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K
Rearranging the ideal gas equation:
• Calculate the partial pressure of CO2:
mass CO2 = 350 g
The molar mass of CO2:
CO2 1 x 12.01 g/mol = 12.01 g/mol
2 x 16.00 g/mol = 32.00 g/mol
Total: 44.01 g/mol
moles CO2 = 7.95 mol CO2
A 36.0–L cylinder of a gas used for calibration of blood gas analyzers in medical laboratories contains 350 g CO2, 805 g O2, and 4,880 g N2. At 25 degrees C, what is the pressure in the cylinder in atmospheres?
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