Pressure atm volume of gas ml 647 ml conclusions 1

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Pressure (atm) Volume of Gas (mL)
64.7 mL Conclusions 1. Which of the gases used in this lab obeyed Boyle’s Law?
2. How would you expect a sample of pentane to behave under similar experimental conditions?
3. Suppose a student plotted the pressure of propane in atm ( y -axis) versus the volume of propane in mL ( x -axis). What shape do you expect the graph to have?
4. Suppose 2.00 atm of an ideal gas occupies a volume of 80 mL. What pressure will the gas have when the volume is expanded to 100 mL?
5. The bubble wrap shown in the figure below is often used to protect fragile objects during shipping. Bubble wrap tends to pop when stepped onto or squeezed. How can you explain this using Boyle’s Law?
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squeezed, the pressure inside the bubbles increase. In fact, the pressure increases so much that the plastic can’t contain it all—which is why it pops. While the pressure is increasing, the volume of the gas is decreases to the point where the gases molecules are going to burst through the plastic. Overall, by pressing the bubble, you are increasing the pressure and decreasing the volume. Page | 5

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