(a) Interpretation: Using the average atomic masses, the mass (in g) of the sample should be determined. 5.0 moles of potassium Concept Introduction: Atomic mass unit measures mass in an atomic scale, it is a standard unit for mass. Here, 1 amu is equal to the mass of either one proton or neutron and equals to 1 g/mol. Atomic mass unit is equal to 1/12 t h of the mass of C-12 atom. For example, if average atomic mass of carbon is 12.01 thus, it is the mass of 1 carbon atom. Number of moles = given mass Molar mass .

BuyFind

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781337399425
BuyFind

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781337399425

Solutions

Chapter 8, Problem 108AP
Interpretation Introduction

(a)

Interpretation:

Using the average atomic masses, the mass (in g) of the sample should be determined.

5.0 moles of potassium

Concept Introduction:

Atomic mass unit measures mass in an atomic scale, it is a standard unit for mass. Here, 1 amu is equal to the mass of either one proton or neutron and equals to 1 g/mol. Atomic mass unit is equal to 1/12th of the mass of C-12 atom. For example, if average atomic mass of carbon is 12.01 thus, it is the mass of 1 carbon atom.

Number of moles = given massMolar mass.

Interpretation Introduction

(b)

Interpretation:

Using the average atomic masses, the mass (in g) of the sample should be determined.

0.000305 mole of mercury

Concept Introduction:

Atomic mass unit measures mass in an atomic scale, it is a standard unit for mass. Here, 1 amu is equal to the mass of either one proton or neutron and equals to 1 g/mol. Atomic mass unit is equal to 1/12th of the mass of C-12 atom. For example, if average atomic mass of carbon is 12.01 thus, it is the mass of 1 carbon atom.

Number of moles = given massMolar mass.

Interpretation Introduction

(c)

Interpretation:

Using the average atomic masses, the mass (in g) of the sample should be determined.

2.31×105 moles of manganese

Concept Introduction:

Atomic mass unit measures mass in an atomic scale, it is a standard unit for mass. Here, 1 amu is equal to the mass of either one proton or neutron and equals to 1 g/mol. Atomic mass unit is equal to 1/12th of the mass of C-12 atom. For example, if average atomic mass of carbon is 12.01 thus, it is the mass of 1 carbon atom.

Number of moles = given massMolar mass.

Interpretation Introduction

(d)

Interpretation:

Using the average atomic masses, the mass (in g) of the sample should be determined.

10.5 moles of phosphorus

Concept Introduction:

Atomic mass unit measures mass in an atomic scale, it is a standard unit for mass. Here, 1 amu is equal to the mass of either one proton or neutron and equals to 1 g/mol. Atomic mass unit is equal to 1/12th of the mass of C-12 atom. For example, if average atomic mass of carbon is 12.01 thus, it is the mass of 1 carbon atom.

Number of moles = given massMolar mass.

Interpretation Introduction

(e)

Interpretation:

Using the average atomic masses, the mass (in g) of the sample should be determined.

4.9×104 moles of iron

Concept Introduction:

Atomic mass unit measures mass in an atomic scale, it is a standard unit for mass. Here, 1 amu is equal to the mass of either one proton or neutron and equals to 1 g/mol. Atomic mass unit is equal to 1/12th of the mass of C-12 atom. For example, if average atomic mass of carbon is 12.01 thus, it is the mass of 1 carbon atom.

Number of moles = given massMolar mass.

Interpretation Introduction

(f)

Interpretation:

Using the average atomic masses, the mass (in g) of the sample should be determined.

125 moles of lithium

Concept Introduction:

Atomic mass unit measures mass in an atomic scale, it is a standard unit for mass. Here, 1 amu is equal to the mass of either one proton or neutron and equals to 1 g/mol. Atomic mass unit is equal to 1/12th of the mass of C-12 atom. For example, if average atomic mass of carbon is 12.01 thus, it is the mass of 1 carbon atom.

Number of moles = given massMolar mass.

Interpretation Introduction

(g)

Interpretation:

Using the average atomic masses, the mass (in g) of the sample should be determined.

0.01205 mole of fluorine

Concept Introduction:

Atomic mass unit measures mass in an atomic scale, it is a standard unit for mass. Here, 1 amu is equal to the mass of either one proton or neutron and equals to 1 g/mol. Atomic mass unit is equal to 1/12th of the mass of C-12 atom. For example, if average atomic mass of carbon is 12.01 thus, it is the mass of 1 carbon atom.

Number of moles = given massMolar mass.

Want to see the full answer?

Check out a sample textbook solution.

Want to see this answer and more?

Experts are waiting 24/7 to provide step-by-step solutions in as fast as 30 minutes!*

*Response times may vary by subject and question complexity. Median response time is 34 minutes for paid subscribers and may be longer for promotional offers.