Table of contents

1. Matter and Measurements4h 29m
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 35m
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. Amines38m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 46m
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

Pressure Units

GOB Chemistry

8. Gases, Liquids and Solids

Pressure Units

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2:34 minutes

Problem 71Timberlake - 13th Edition

Textbook Question

In 1783, Jacques Charles launched his first balloon filled with hydrogen gas, which he chose because it was lighter than air. If the balloon had a volume of 31 000 L, how many kilograms of hydrogen were needed to fill the balloon at STP? (8.6)

Verified step by step guidance

Identify the conditions of STP (Standard Temperature and Pressure), which are 0°C (273.15 K) and 1 atm pressure.

Use the ideal gas law equation, PV = nRT, to find the number of moles of hydrogen gas (H₂). Here, P is pressure, V is volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is temperature in Kelvin.

Substitute the given values into the ideal gas law equation: P = 1 atm, V = 31,000 L, R = 0.0821 L·atm/mol·K, and T = 273.15 K.

Solve the equation for n (number of moles of hydrogen gas): n = PV / RT.

Convert the number of moles of hydrogen gas to mass in kilograms using the molar mass of hydrogen (H₂), which is approximately 2.02 g/mol. Remember to convert grams to kilograms by dividing by 1,000.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ideal Gas Law

The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of a gas. It is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. This law allows us to calculate the amount of gas needed under specific conditions, such as Standard Temperature and Pressure (STP).

Standard Temperature and Pressure (STP)

Standard Temperature and Pressure (STP) is a reference point used in chemistry to define the conditions under which gas calculations are made. STP is defined as a temperature of 0 degrees Celsius (273.15 K) and a pressure of 1 atmosphere (101.3 kPa). At STP, one mole of an ideal gas occupies 22.4 liters, which is crucial for determining the number of moles of hydrogen gas needed to fill the balloon.

Molar Mass of Hydrogen

The molar mass of hydrogen is the mass of one mole of hydrogen gas (H2), which is approximately 2 grams per mole. This value is essential for converting the number of moles of hydrogen gas calculated from the Ideal Gas Law into grams or kilograms. Understanding the molar mass allows us to determine how much hydrogen is required to fill the balloon to the specified volume at STP.