(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 .

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Answer 1

Question

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 1/12^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 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 1/12^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 massMolar mass.

Interpretation Introduction

(c)

Interpretation:

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

2.31×10−5 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 1/12^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 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 1/12^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 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 1/12^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 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 1/12^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 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 1/12^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 massMolar mass.

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(5pts) Provide the complete arrow pushing mechanism for the chemical transformation depicted below Use proper curved arrow notation that explicitly illustrates all bonds being broken, and all bonds formed in the transformation. Also, be sure to include all lone pairs and formal charges on all atoms involved in the flow of electrons. CH3O H I I CH3O-H H I ① H

6. Draw the products) formed from the following reactions. (a) HI

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Answer 2

Question

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 1/12^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 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 1/12^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 massMolar mass.

Interpretation Introduction

(c)

Interpretation:

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

2.31×10−5 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 1/12^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 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 1/12^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 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 1/12^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 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 1/12^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 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 1/12^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 massMolar mass.

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Answer 3

Question

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 1/12^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 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 1/12^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 massMolar mass.

Interpretation Introduction

(c)

Interpretation:

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

2.31×10−5 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 1/12^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 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 1/12^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 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 1/12^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 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 1/12^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 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 1/12^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 massMolar mass.

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Answer 4

Question

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 1/12^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 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 1/12^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 massMolar mass.

Interpretation Introduction

(c)

Interpretation:

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

2.31×10−5 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 1/12^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 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 1/12^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 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 1/12^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 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 1/12^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 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 1/12^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 massMolar mass.

Expert Solution & Answer

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Check out a sample textbook solution

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Answer 5

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 1/12^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 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 1/12^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 massMolar mass.

Interpretation Introduction

(c)

Interpretation:

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

2.31×10−5 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 1/12^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 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 1/12^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 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 1/12^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 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 1/12^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 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 1/12^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 massMolar mass.

Answer 6

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 1/12^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 massMolar mass.

Answer 7

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 1/12^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 massMolar mass.

Answer 8

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 1/12^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 massMolar mass.

Answer 9

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 1/12^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 massMolar mass.

Answer 10

Interpretation Introduction

(c)

Interpretation:

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

2.31×10−5 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 1/12^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 massMolar mass.

Answer 11

Interpretation Introduction

(c)

Interpretation:

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

2.31×10−5 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 1/12^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 massMolar mass.

Answer 12

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 1/12^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 massMolar mass.

Answer 13

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 1/12^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 massMolar mass.

Answer 14

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 1/12^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 massMolar mass.

Answer 15

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 1/12^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 massMolar mass.

Answer 16

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 1/12^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 massMolar mass.

Answer 17

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 1/12^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 massMolar mass.

Answer 18

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 1/12^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 massMolar mass.

Answer 19

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 1/12^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 massMolar mass.

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Solution Summary: The author explains how the average atomic masses determine the mass (in g) of the sample.

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