Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

8. Gases, Liquids and Solids

Standard Temperature and Pressure

GOB Chemistry

8. Gases, Liquids and Solids

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

First, understand that STP (Standard Temperature and Pressure) conditions are defined as 0°C (273.15 K) and 1 atm pressure. At STP, 1 mole of any ideal gas occupies 22.4 liters.

Next, 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 4.00 g/mol, Neon (Ne) is approximately 20.18 g/mol, and Nitrogen (N) is approximately 14.01 g/mol.

Calculate the moles for each gas: For Helium, \( \text{moles of He} = \frac{10.0 \text{ g}}{4.00 \text{ g/mol}} \). For Neon, \( \text{moles of Ne} = \frac{10.0 \text{ g}}{20.18 \text{ g/mol}} \). For Nitrogen, \( \text{moles of N} = \frac{10.0 \text{ g}}{14.01 \text{ g/mol}} \).

Finally, compare the number of moles calculated for each gas. The gas with the highest number of moles will have the greatest volume at STP, since volume is directly proportional to the number of moles under these conditions.