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

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5:06 minutes

Problem 80c

Textbook Question

Using the models of the molecules (black = C, white = H, yellow = S, red = O), determine each of the following for models of compounds 1 and 2:

c. number of moles in 10.0 g

Verified step by step guidance

Step 1: Identify the molecular formula for each compound based on the color-coded atoms in the models. For compound 1, the molecule consists of sulfur (yellow), oxygen (red), and hydrogen (white). For compound 2, the molecule includes carbon (black), hydrogen (white), and nitrogen (blue).

Step 2: Determine the molar mass of each compound by summing the atomic masses of all atoms in the molecular formula. Use the periodic table to find the atomic masses: Carbon (C) = 12.01 g/mol, Hydrogen (H) = 1.008 g/mol, Sulfur (S) = 32.07 g/mol, Oxygen (O) = 16.00 g/mol, and Nitrogen (N) = 14.01 g/mol.

Step 3: Calculate the number of moles in 10.0 g of each compound using the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \). Substitute the given mass (10.0 g) and the molar mass calculated in Step 2.

Step 4: Perform dimensional analysis to ensure the units cancel appropriately, leaving the result in moles. This step confirms the calculation is set up correctly.

Step 5: Interpret the results to understand the number of moles for each compound. This value represents the quantity of molecules present in 10.0 g of the substance.

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Key Concepts

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

Molecular Composition

Molecular composition refers to the types and numbers of atoms present in a molecule. In the context of the question, understanding the molecular formulas of compounds 1 and 2 is essential for determining their properties and behaviors in chemical reactions. The colors in the models represent different elements: black for carbon (C), white for hydrogen (H), yellow for sulfur (S), and red for oxygen (O).

Moles and Molar Mass

A mole is a unit in chemistry that represents 6.022 x 10²³ particles (atoms, molecules, etc.). Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To find the number of moles in a given mass (like 10.0 g), one must divide the mass by the molar mass of the compound. This concept is crucial for quantifying substances in chemical reactions.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions. It involves using the balanced chemical equation to determine the relationships between the amounts of substances involved. In this question, stoichiometry will help in understanding how the number of moles of each compound relates to the overall reaction and how to calculate the moles from the given mass.