   # What amount (moles) of compound is present in 1.00 g of each of the compounds in Exercise 51? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 5, Problem 53E
Textbook Problem
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## What amount (moles) of compound is present in 1.00 g of each of the compounds in Exercise 51?

(a)

Interpretation Introduction

Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.

The amount of substance containing 12g of pure carbon is called a mole. One mole of atoms always contains 6.022×1023 atoms. The number of moles is also called Avogadro’s number.

Hence,

(6.022×1023 atoms)(12u1atom)=12g1u=16.022×1023 g

Also, the formula of number of moles is,

Molesofatom=massofatomatomicmass

To determine: The amount (moles) of compound in 1.00g of NH3 .

### Explanation of Solution

Given

The given mass of NH3 is 1.00g .

The molar mass of NH3 is,

3.0237g/mol+14.006g/mol=17.0297g/mol

The amount of compound NH3 is 1.00g is calculated as,

MolesofNH3atom=massofNH3

(b)

Interpretation Introduction

Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.

The amount of substance containing 12g of pure carbon is called a mole. One mole of atoms always contains 6.022×1023 atoms. The number of moles is also called Avogadro’s number.

Hence,

(6.022×1023 atoms)(12u1atom)=12g1u=16.022×1023 g

Also, the formula of number of moles is,

Molesofatom=massofatomatomicmass

To determine: The amount (moles) of compound in 1.00g of N2H4 .

(c)

Interpretation Introduction

Concept introduction: The atomic mass is defined as the sum of number of protons and

Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.

The amount of substance containing 12g of pure carbon is called a mole. One mole of atoms always contains 6.022×1023 atoms. The number of moles is also called Avogadro’s number.

Hence,

(6.022×1023 atoms)(12u1atom)=12g1u=16.022×1023 g

Also, the formula of number of moles is,

Molesofatom=massofatomatomicmass

To determine: The amount (moles) of compound in 1.00g of (NH4)2Cr2O7 .

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