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

1:22 minutes

Problem 34

Textbook Question

Find the mass in atomic mass units of the following:
a. 1 O atom, with a mass of 2.66 × 10^-23 g
b. 1 Br atom, with a mass of 1.31 × 10^-22 g

Verified step by step guidance

Step 1: Recall the relationship between atomic mass units (amu) and grams. By definition, 1 amu = 1.660539066 × 10^-24 g.

Step 2: For part (a), calculate the mass of 1 O atom in amu by dividing its given mass in grams (2.66 × 10^-23 g) by the conversion factor (1.660539066 × 10^-24 g/amu). Use the formula:

\frac{2.66 \times 10^{- 23}}{1.660539066 \times 10^{- 24}}

Step 3: For part (b), calculate the mass of 1 Br atom in amu using the same method. Divide its given mass in grams (1.31 × 10^-22 g) by the conversion factor (1.660539066 × 10^-24 g/amu). Use the formula:

\frac{1.31 \times 10^{- 22}}{1.660539066 \times 10^{- 24}}

Step 4: Simplify the results for both calculations by performing the division and adjusting the powers of 10 as needed. This will give you the mass of each atom in amu.

Step 5: Verify your results by checking the units and ensuring the calculations align with the relationship between grams and amu.

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.

Atomic Mass Unit (amu)

An atomic mass unit (amu) is a standard unit of mass that quantifies mass on an atomic or molecular scale. It is defined as one twelfth of the mass of a carbon-12 atom, approximately 1.66 x 10^-24 grams. This unit is essential for comparing the masses of different atoms and molecules, allowing for easier calculations in chemistry.

Conversion from grams to amu

To convert the mass of an atom from grams to atomic mass units, one must use the conversion factor that 1 amu is approximately equal to 1.66 x 10^-24 grams. This involves dividing the mass in grams by this conversion factor, enabling the expression of atomic masses in a more manageable unit that is commonly used in chemistry.

Mass of Elements

The mass of elements, such as oxygen (O) and bromine (Br), is a fundamental property that influences their behavior in chemical reactions. Each element has a specific atomic mass, which can be found on the periodic table. Understanding the mass of individual atoms is crucial for stoichiometry, which involves calculating the quantities of reactants and products in chemical reactions.

Watch next

Master Mole Concept with a bite sized video explanation from Jules

Start learning

Related Videos

Related Practice

Textbook Question

Calculate the mass, in grams, for each of the following:

d. 0.145 mole of C₂H₆O

1210

views

Textbook Question

How many Na⁺ ions are in a mole of Na₂SO₄? How many SO₄^2- ions?

1585

views

Textbook Question

How many moles of ions are in 1.75 mol of K₂SO₄?

Caffeine has the formula C₈H₁₀N₄O₂. If an average cup of coffee contains approximately 125 mg of caffeine, how many moles of caffeine are in one cup?

1972

views

Textbook Question

The principal component of many kidney stones is calcium oxalate, CaC₂O₄. A kidney stone recovered from a typical patient contains 8.5 × 10²⁰ formula units of calcium oxalate. How many moles of CaC₂O₄ are present in this kidney stone? What is the mass of the kidney stone in grams?

1885

views

Textbook Question

How many O atoms of mass 15.99 amu are in 15.99 g of oxygen?

1381

views

Textbook Question

Calcium citrate, Ca(C₆H₅O₇)₂(MW = 498.5 amu), is a common dietary supplement to provide calcium needed for strong teeth and bones.

b. What mass of calcium citrate would be needed to provide the recommended daily intake of calcium?

1672

views

Textbook Question

Obtain a bottle of aspirin and identify the amount of active ingredient (acetylsalicylic acid, C₉H₈O₄) per tablet.

a. How many moles of aspirin are in one tablet?

1221

views

Show more practices

Download the Mobile app

Privacy

Do not sell my personal information

Accessibility

Patent notice

Sitemap

Find the mass in atomic mass units of the following: a. 1 O atom, with a mass of 2.66 × 10-23 g b. 1 Br atom, with a mass of 1.31 × 10-22 g

Key Concepts

Atomic Mass Unit (amu)

Conversion from grams to amu

Mass of Elements

Watch next

Find the mass in atomic mass units of the following:
a. 1 O atom, with a mass of 2.66 × 10^-23 g
b. 1 Br atom, with a mass of 1.31 × 10^-22 g