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A cylinder of O2(g) used in breathing by emphysema patients has a volume of 5.00 L at a pressure of 19.0 atm. If the temperature of the cylinder is 33.3°C, what mass (in g) of oxygen is in the cylinder?

Question

A cylinder of O2(g) used in breathing by emphysema patients has a volume of 5.00 L at a pressure of 19.0 atm. If the temperature of the cylinder is 33.3°C, what mass (in g) of oxygen is in the cylinder?

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Solution

To solve this problem, we will use the ideal gas law equation, which is PV = nRT.

Here's the step-by-step solution:

  1. Convert the temperature from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = °C + 273.15. So, 33.3°C = 33.3 + 273.15 = 306.45 K.

  2. Rearrange the ideal gas law equation to solve for n (number of moles). The rearranged equation is n = PV/RT.

  3. Plug in the given values into the equation. The pressure P is 19.0 atm, the volume V is 5.00 L, the gas constant R is 0.0821 L·atm/K·mol (this is the value of R that should be used when pressure is in atm and volume is in liters), and the temperature T is 306.45 K. So, n = (19.0 atm * 5.00 L) / (0.0821 L·atm/K·mol * 306.45 K) = 3.00 mol.

  4. Now, we need to convert moles of O2 to grams. The molar mass of O2 is approximately 32.00 g/mol. So, the mass of O2 is 3.00 mol * 32.00 g/mol = 96.0 g.

So, the mass of oxygen in the cylinder is 96.0 g.

This problem has been solved

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