# What is the mass of each sample? a.2.75 mol Fe b.0.115 mol Al c.125 mol Si d.1 Ni 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 48E
Textbook Problem
364 views

## What is the mass of each sample?a.2.75 mol Feb.0.115 mol Alc.125 mol Sid.1 Ni atom

Interpretation Introduction

Interpretation:

The mass of each 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) 2.75 mole Fe

The mass of Fe is calculated as follows:

The molar mass of Fe is 55.84 g.

Mass of 1 mole of Fe = 55.84 gMass of 2.75 mole of Fe = 55.84 g1mole ×2.75mole                                      = 154 g

Therefore, the mass of Fe is 154 g

b) 0.115 moles Al

The mass of Al is calculated as follows:

The molar mass of Al is 27 g.

Mass of 1 mole of Al = 27 gMass of 0.115 moles of Al = 27 g1mole ×0.115mole                                      = 3.10 g

Thus, the mass of Al is 3.10 g.

c) 125 moles Si

The mass of Si is calculated as follows:

The molar mass of Si is 28.1 g.

Mass of 1 mole of Si = 28.1 gMass of 125 moles of Si = 28.1 g1mole ×125mole                                      = 35.1×103 g

Hence, the mass of Si is 35

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