# What is the mass of each sample? a.1.8 mol S b.0.0067 mol Au c.0.552 mol Cu d.1 Na atom

### Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692

Chapter
Section

### Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 3, Problem 47E
Textbook Problem
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## What is the mass of each sample?a.1.8 mol Sb.0.0067 mol Auc.0.552 mol Cud.1 Na atom

Interpretation Introduction

Interpretation:

The mass of each given sample is to be calculated.

Concept Introduction:

 A mole is a unit of amount of substance. It relates the number of particles to the molar mass.

 One mole of a substance contains Avogadro’s number that is 6.022×1023 particles. The number remains constant regardless of the nature of the substance. One mole of an atom contains 6.022×1023 atoms. One mole of molecules contains 6.022×1023 molecules.

 It also relates to the molar mass of a substance in grams. One mole of a substance weighs that amount in grams which is equal to its molar mass.

### Explanation of Solution

a) 1.8 moles S

The mass of S is calculated as follows:

The molar mass of S is 32.06 g.

Mass of 1 mole of S = 32.06 gMass of 1.8 mole of S = 32.06 g1mole ×1.8mole                                      = 58 g S

Hence, the mass of S is 58 g.

b) 0.0067 moles Au

The mass of Au is calculated as follows:

The molar mass of Au is 196.97 g.

Mass of 1 mole of Au = 197 gMass of 0.0067 moles of Au = 196.97 g1mole ×0.0067mole1                                      = 1.3 g

Therefore, the mass of Au is 1.3 g .

c)0.552 moles Cu

The mass of Cu is calculated as follows:

The molar mass of Cu is 63.55 g.

Mass of 1 mole of Cu = 63.55 gMass of 0

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