The molecular formula of the compound with empirical formula CH 2 and molar mass 42.08 g/mol is to be determined. Concept introduction: An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule. Following are the steps to determine the molecular formula of a compound. Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound. Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows: Whole − number multiple = Molar mass of compound Empirical formula mass (1) Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

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Answer 1

Question

Chapter 3, Problem 3.40P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH2 and molar mass 42.08 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(b)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NH2 and molar mass 32.05 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(c)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NO2 and molar mass 92.02 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(d)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CHN and molar mass 135.14 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

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Part II. Identify whether the two protons in blue are homotopic, enantiopic, diasteriotopic, or heterotopic. a) HO b) Bri H HH c) d) H H H Br 0

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Answer 2

Question

Chapter 3, Problem 3.40P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH2 and molar mass 42.08 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(b)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NH2 and molar mass 32.05 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(c)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NO2 and molar mass 92.02 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(d)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CHN and molar mass 135.14 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

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Answer 3

Question

Chapter 3, Problem 3.40P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH2 and molar mass 42.08 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(b)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NH2 and molar mass 32.05 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(c)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NO2 and molar mass 92.02 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(d)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CHN and molar mass 135.14 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

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Answer 4

Question

Chapter 3, Problem 3.40P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH2 and molar mass 42.08 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(b)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NH2 and molar mass 32.05 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(c)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NO2 and molar mass 92.02 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(d)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CHN and molar mass 135.14 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

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Answer 5

Chapter 3, Problem 3.40P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH2 and molar mass 42.08 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(b)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NH2 and molar mass 32.05 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(c)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NO2 and molar mass 92.02 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

(d)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CHN and molar mass 135.14 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

Answer 6

Chapter 3, Problem 3.40P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH2 and molar mass 42.08 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

Answer 7

Chapter 3, Problem 3.40P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH2 and molar mass 42.08 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NH2 and molar mass 32.05 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NH2 and molar mass 32.05 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NO2 and molar mass 92.02 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula NO2 and molar mass 92.02 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

Answer 12

(d)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CHN and molar mass 135.14 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

Answer 13

(d)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CHN and molar mass 135.14 g/mol is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

Following are the steps to determine the molecular formula of a compound.

Step 1: Add the molar mass of each element multiplied by its number of atoms present in the empirical formula to obtain the empirical formula mass for the compound.

Step 2: Divide the molar mass of the compound by its empirical formula mass to obtain the whole number. The formula to calculate the whole number multiple is as follows:

Whole−number multiple=Molar mass of compoundEmpirical formula mass (1)

Step 3: Multiply the whole number with the subscript of each element present in the empirical formula. This gives the molecular formula of the compound.

Answer 14

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Answer 15

Expert Solution & Answer

Answer 16

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Answer 17

Ch. 3.1 - Graphite is the crystalline form of carbon used in...Ch. 3.1 - Prob. 3.1BFP Ch. 3.1 - At rest, a person inhales 9.72×1021 nitrogen...Ch. 3.1 - Prob. 3.2BFP Ch. 3.1 - Prob. 3.3AFP Ch. 3.1 - Prob. 3.3BFP Ch. 3.1 - Fluoride ion is added to drinking water to prevent...Ch. 3.1 - Calcium chloride is applied to highways in winter...Ch. 3.1 - Tetraphosphorus decoxide reacts with water to form...Ch. 3.1 - Prob. 3.5BFP

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