Table of contents

1. The Chemical World9m
- The Scientific Method
  9m
2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
6. Chemical Composition1h 23m
7. Chemical Reactions1h 43m
8. Quantities in Chemical Reactions1h 8m
9. Electrons in Atoms and the Periodic Table2h 32m
10. Chemical Bonding2h 10m
11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
13. Solutions3h 1m
14. Acids and Bases2h 14m
15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

11 Gases

The Ideal Gas Law Derivations

Introduction to Chemistry

11 Gases

The Ideal Gas Law Derivations

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Multiple Choice

A cylinder with a movable piston contains 0.615 moles of gas and has a volume of 295 mL. What will its volume be if 0.103 moles of gas escaped?

0.176 L

0.217 L

0.246 L

0.361 L

1.28 L

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Verified step by step guidance

Identify the initial conditions: The cylinder contains 0.615 moles of gas with a volume of 295 mL.

Determine the final amount of gas: Subtract the moles of gas that escaped (0.103 moles) from the initial moles (0.615 moles) to find the remaining moles of gas.

Use the ideal gas law concept: Since the pressure and temperature are constant, use the relationship \( V_1 / n_1 = V_2 / n_2 \), where \( V_1 \) and \( n_1 \) are the initial volume and moles, and \( V_2 \) and \( n_2 \) are the final volume and moles.

Rearrange the equation to solve for the final volume \( V_2 \): \( V_2 = V_1 \times (n_2 / n_1) \).

Substitute the known values into the equation: \( V_2 = 295 \text{ mL} \times ((0.615 - 0.103) / 0.615) \) and convert the final volume from mL to L by dividing by 1000.