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

6. Chemical Reactions & Quantities

Mole Concept

GOB Chemistry

6. Chemical Reactions & Quantities

Mole Concept

Previous problemNext problem

3:13 minutes

Problem 6

Textbook Question

Which weighs more, 5.00 g or 0.0225 mol of acetaminophen (C₈H₉O₂)?

Verified step by step guidance

Step 1: Calculate the molar mass of acetaminophen (C8H9O2). Add the atomic masses of all the atoms in the molecular formula: (8 × atomic mass of C) + (9 × atomic mass of H) + (2 × atomic mass of O). Use the periodic table to find the atomic masses of C, H, and O.

Step 2: Multiply the molar mass of acetaminophen by the given number of moles (0.0225 mol) to find the mass of 0.0225 mol of acetaminophen. Use the formula: mass = moles × molar mass.

Step 3: Compare the calculated mass of 0.0225 mol of acetaminophen to the given mass of 5.00 g. Determine which value is greater.

Step 4: Conclude which quantity weighs more based on the comparison in Step 3.

Step 5: Ensure all units are consistent and properly labeled throughout the calculations to avoid errors.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above

Video duration:

Play a video:

Was this helpful?

Key Concepts

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

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For acetaminophen (C8H9O2), the molar mass can be calculated by summing the atomic masses of its constituent elements: carbon (C), hydrogen (H), and oxygen (O). This value is essential for converting between grams and moles, allowing us to determine the weight of a given amount of substance.

Conversion Between Grams and Moles

To compare weights in grams and moles, one must convert moles to grams using the molar mass. The formula used is: mass (g) = number of moles × molar mass (g/mol). This conversion is crucial for answering the question, as it allows for a direct comparison between the given weight of 5.00 g and the weight of 0.0225 mol of acetaminophen.

Comparative Weight Analysis

Comparative weight analysis involves evaluating two or more quantities to determine which is greater. In this context, after converting 0.0225 mol of acetaminophen to grams using its molar mass, one can directly compare the resulting weight to the fixed weight of 5.00 g. This analysis is fundamental to answering the question accurately.

Watch next

Master Mole Concept with a bite sized video explanation from Jules

Start learning

Related Videos

Related Practice

Multiple Choice

A cylindrical copper wire is used for the fences around a house. The copper wire has a diameter of 0.0750 in. How many copper atoms are found in 5.160 cm piece? The density of copper is 8.96 g/cm³. (V = π • r² • h)

The density of the sun is 1.41 g/cm³ and its volume is 1.41 x 10²⁷ m³. How many hydrogen molecules are in the sun if we assume all the mass is hydrogen gas?

What is a mole?

What is Avogadro's number?

2309

views

Textbook Question