The molecular formula of the compound with empirical formula CH and molar mass 78.11 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound. 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 3.41P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH and molar mass 78.11 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C3H6O2 and molar mass 74.08 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 HgCl and molar mass 472.1 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C7H4O2 and molar mass 240.20 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 2

Question

Chapter 3, Problem 3.41P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH and molar mass 78.11 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C3H6O2 and molar mass 74.08 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 HgCl and molar mass 472.1 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C7H4O2 and molar mass 240.20 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 3.41P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH and molar mass 78.11 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C3H6O2 and molar mass 74.08 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 HgCl and molar mass 472.1 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C7H4O2 and molar mass 240.20 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 3.41P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH and molar mass 78.11 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C3H6O2 and molar mass 74.08 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 HgCl and molar mass 472.1 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C7H4O2 and molar mass 240.20 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 3.41P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH and molar mass 78.11 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C3H6O2 and molar mass 74.08 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 HgCl and molar mass 472.1 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C7H4O2 and molar mass 240.20 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 3.41P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH and molar mass 78.11 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 3.41P

(a)

Interpretation Introduction

Interpretation:

The molecular formula of the compound with empirical formula CH and molar mass 78.11 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C3H6O2 and molar mass 74.08 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C3H6O2 and molar mass 74.08 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 HgCl and molar mass 472.1 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 HgCl and molar mass 472.1 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 compound. The molecular formula tells the exact number of atoms of each element present in a compound.

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 C7H4O2 and molar mass 240.20 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 C7H4O2 and molar mass 240.20 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

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Answer 16

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Answer 17

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