Problem: 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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FREE Expert Solution

We’re going to calculate the pressure of each gas first using the ideal gas equation:

PV=nRT

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:

PVV=nRTVP=nRTV



 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=350.0 g CO2×1 mol CO244.01 g O2

  moles CO2 = 7.95 mol CO2

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Problem Details

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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Our tutors have indicated that to solve this problem you will need to apply the Partial Pressure concept. You can view video lessons to learn Partial Pressure. Or if you need more Partial Pressure practice, you can also practice Partial Pressure practice problems.

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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.