🤓 Based on our data, we think this question is relevant for Professor Asala's class at UNC.
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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Based on our data, we think this problem is relevant for Professor Asala's class at UNC.
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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.