   Chapter 3, Problem 59E

Chapter
Section
Textbook Problem

What mass of nitrogen is present in 5.00 moles of each of the compounds in Exercise 51?

(a)

Interpretation Introduction

Interpretation: The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 is to be determined.

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

Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.

The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.

The amount of substance containing 12g of pure carbon is called a mole. One mole of substance always contains 6.022×1023 atoms.

Hence,

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

To determine: The mass of nitrogen (N) in 5.00 moles of NH3 .

Explanation

Given

The moles of NH3 is 5.00 .

Since, one mole of NH3 is equal to one mole of nitrogen, Therefore, 5.00 moles of NH3 is equal to 5.00 moles of nitrogen (N) .

The atomic mass of nitrogen (N) is 14.006g/mol .

Formula

The mass of nitrogen (N) in NH3 is calculated using the formula,

MolesofN=MassofNAtomic

(b)

Interpretation Introduction

Interpretation: The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 is to be determined.

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

Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.

The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.

The amount of substance containing 12g of pure carbon is called a mole. One mole of substance always contains 6.022×1023 atoms.

Hence,

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

To determine: The mass of nitrogen (N) in 5.00 moles of N2H4 .

(c)

Interpretation Introduction

Interpretation: The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 is to be determined.

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

Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.

The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.

The amount of substance containing 12g of pure carbon is called a mole. One mole of substance always contains 6.022×1023 atoms.

Hence,

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

To determine: The mass of nitrogen (N) in 5.00 moles of (NH4)2Cr2O7 .

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