A sealed cylindrical container of height 1.5 m and radius 0.3 m is filled with dry air at 1 atm and 0°C. How many moles of air are in the container? (Assume molar volume at STP = 22.4 L/mol).

Step-by-step solution

1. 1. Compute the volume of the cylinder: $V=\pi r^{2}h=\pi (0.3{)}^2(1.5)$.
2. 2. Evaluate: $V=\pi (0.09)(1.5)=0.424m^3$.
3. 3. Convert to litres: $0.424m^3=424L$.
4. 4. Number of moles = $\frac{424L}{22.4L/mol}=18.93mol$.
5. 5. Round to nearest whole number: 19 mol.
6. Thus the container contains about 19 moles of air.

Concept tested: Moles of air in a given volume

Published 1 October 2026 · How this solution was prepared and checked