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

Standard Temperature and Pressure

Introduction to Chemistry

11 Gases

Standard Temperature and Pressure

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Multiple Choice

Which gas sample has the greatest volume at STP?

10.0 g He

10.0 g Ne

10.0 g N

All have the same volume

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Verified step by step guidance

Understand that STP (Standard Temperature and Pressure) conditions are defined as 0 degrees Celsius and 1 atm pressure, where 1 mole of any ideal gas occupies 22.4 liters.

Calculate the number of moles for each gas sample using the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).

Determine the molar mass of each gas: Helium (He) is approximately 4 g/mol, Neon (Ne) is approximately 20 g/mol, and Nitrogen (N) is approximately 14 g/mol.

Calculate the moles for each gas: For Helium, \( \text{moles of He} = \frac{10.0 \text{ g}}{4 \text{ g/mol}} \); for Neon, \( \text{moles of Ne} = \frac{10.0 \text{ g}}{20 \text{ g/mol}} \); for Nitrogen, \( \text{moles of N} = \frac{10.0 \text{ g}}{14 \text{ g/mol}} \).

Compare the number of moles for each gas to determine which has the greatest volume at STP, as the volume is directly proportional to the number of moles.