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Chemistry

10th Edition
Steven S. Zumdahl + 2 others
ISBN: 9781305957404

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BuyFindarrow_forward

Chemistry

10th Edition
Steven S. Zumdahl + 2 others
ISBN: 9781305957404
Textbook Problem

Dimethylnitrosamine, (CH3)2N2O , is a carcinogenic (cancer-causing) substance that may be formed in foods, beverages, or gastric juices from the reaction of nitrite ion (used as a food preservative) with other substances.

a. What is the molar mass of dimethylnitrosamine?

b. How many moles of (CH3h N20 molecules are present in 250 mg dimethylnitrosamine?

c. What is the mass of 0.050 mole of dimethylnitrosamine?

d. How many atoms of hydrogen are in 1.0 mole of dimethylnitrosamine?

e. What is the mass of 1.0 × 106 molecules of dimethylnitrosamine?

f. What is the mass in grams of one molecule of dimethylnitrosamine?

(a)

Interpretation Introduction

Interpretation: The answers are to be given for the given options.

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 atoms always contains 6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.

Explanation

To determine: The molar mass of Dimethylnitrosamine [(CH3)2N2O] .

The atomic weight of carbon (C) is 12.01g/mol .

The atomic weight of oxygen (O) is 16.00g/mol .

The atomic weight of hydrogen (H) is 1.008g/mol .

The atomic weight of nitrogen (N) is 14.01g/mol .

In a compound (CH3)2N2O , two carbon, one oxygen, two nitrogen and six hydrogen atoms are present. Hence, molar mass of (CH3)2N2O is calculated as,

[6(1

(b)

Interpretation Introduction

Interpretation: The answers are to be given for the given options.

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 atoms always contains 6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.

To determine: The number of moles in 250mg of (CH3)2N2O .

(c)

Interpretation Introduction

Interpretation: The answers are to be given for the given options.

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 atoms always contains 6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.

To determine: The mass of 0.050mol (CH3)2N2O .

(d)

Interpretation Introduction

Interpretation: The answers are to be given for the given options.

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 atoms always contains 6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.

To determine: The number of hydrogen (H) atoms in 1.00mol of (CH3)2N2O .

(e)

Interpretation Introduction

Interpretation: The answers are to be given for the given options.

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 atoms always contains 6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.

To determine: The mass of exactly 1.0×106molecules of (CH3)2N2O .

(f)

Interpretation Introduction

Interpretation: The answers are to be given for the given options.

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 atoms always contains 6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.

To determine: The mass of exactly 1.0molecules of (CH3)2N2O .

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