A sample of oxygen gas contains 15.0 mol in a volume of 23.5 L . If the pressure and temperature are kept constant, but the volume is changed to 6.10 L , how many moles of oxygen gas does the sample contain? Be sure your answer has the correct number of significant figures.

When dealing with the relationship between pressure, volume, and number of moles, Boyle's Law can be applied, which states that \( P_1V_1 = P_2V_2 \). Since pressure and temperature are constant, you can use the equation \(\frac{n_1}{V_1} = \frac{n_2}{V_2}\). Rearranging gives \( n_2 = n_1 \times \frac{V_2}{V_1} \). Substituting values, we get \( n_2 = 15.0 \, \text{mol} \times \frac{6.10 \, \text{L}}{23.5 \, \text{L}} \approx 3.91 \, \text{mol} \). Thus, the sample contains 3.91 mol of oxygen gas, when rounded to three significant figures. In the context of gas laws, it’s fascinating how the behavior of gases can lead us to predict their movement during various conditions. Gas laws not only aid in scientific endeavors but also play a vital role in industries like pharmaceuticals and materials engineering, where understanding gas reactions and behaviors can optimize production processes and ensure safety. Knowing how to manipulate these variables opens up a world of possibilities for innovation!