/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 66 Dimethylnitrosamine, \(\left(\ma... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 3: Problem 66

Dimethylnitrosamine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{~N}_{2} \mathrm{O}\), is a carcinogenic (cancercausing) 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 \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{~N}_{2} \mathrm{O}\) molecules are present in \(250 \mathrm{mg}\) dimethylnitrosamine? c. What is the mass of \(0.050\) mol dimethylnitrosamine? d. How many atoms of hydrogen are in \(1.0 \mathrm{~mol}\) dimethylnitrosamine? e. What is the mass of \(1.0 \times 10^{6}\) molecules of dimethylnitrosamine? f. What is the mass in grams of one molecule of dimethylnitrosamine?

Short Answer

Expert verified
a. The molar mass of dimethylnitrosamine is 74.14 g/mol. b. There are 3.37 x 10^(-3) moles of dimethylnitrosamine in 250 mg. c. The mass of 0.050 mol dimethylnitrosamine is 3.71 g. d. There are 3.613 x 10^(24) hydrogen atoms in 1.0 mol of dimethylnitrosamine. e. The mass of 1.0 x 10^6 molecules of dimethylnitrosamine is 1.23 x 10^(-16) g. f. The mass of one molecule of dimethylnitrosamine is 1.23 x 10^(-22) g.

Step by step solution

01

Determine chemical formula and atomic masses

The molecular formula for dimethylnitrosamine is \((CH_3)_2N_2O\). The atomic masses (in g/mol) are: - Carbon (C): 12.01 - Hydrogen (H): 1.01 - Nitrogen (N): 14.01 - Oxygen (O): 16.00
02

Calculate molar mass

To find the molar mass of dimethylnitrosamine, we'll add the atomic masses of each atom considering the number of atoms: Molar mass = 2(12.01) + 6(1.01) + 2(14.01) + 1(16.00) = 74.14 g/mol. The molar mass of dimethylnitrosamine is 74.14 g/mol. #b. Calculate moles of dimethylnitrosamine in 250 mg#
03

Convert mass to grams

First, convert the mass of dimethylnitrosamine to grams: 250 mg = 0.250 g.
04

Calculate moles from mass and molar mass

To calculate the moles: Moles = (Mass) / (Molar mass) = 0.250 g / 74.14 g/mol = 3.37 x 10^(-3) moles. There are 3.37 x 10^(-3) moles of dimethylnitrosamine in 250 mg. #c. Calculate the mass of 0.050 mol dimethylnitrosamine#
05

Calculate mass from moles and molar mass

To calculate the mass: Mass = (Moles) x (Molar mass) = 0.050 mol x 74.14 g/mol = 3.71 g. The mass of 0.050 mol dimethylnitrosamine is 3.71 g. #d. Calculate the number of hydrogen atoms in 1.0 mol dimethylnitrosamine#
06

Calculate the hydrogen atoms in one molecule

In one molecule of dimethylnitrosamine, there are six hydrogen atoms (two methyl groups, each having three hydrogens).
07

Calculate the total hydrogen atoms

Since there are 6 hydrogen atoms per molecule and 1.0 mol of dimethylnitrosamine: Total hydrogen atoms = 6 (hydrogen atoms) x 1.0 (moles) x \(6.022 \times 10^{23}\) (Avogadro's number). Total hydrogen atoms = 3.613 x 10^(24) hydrogen atoms. There are 3.613 x 10^(24) hydrogen atoms in 1.0 mol of dimethylnitrosamine. #e. Calculate the mass of 1.0 x 10^6 molecules of dimethylnitrosamine#
08

Calculate moles from number of molecules

To calculate moles from number of molecules, use Avogadro's number: Moles = \(1.0 \times 10^{6}\) molecules / \(6.022 \times 10^{23}\) molecules/mol = 1.66 x 10^(-18) moles.
09

Calculate mass from moles and molar mass

To calculate the mass: Mass = (Moles) x (Molar mass) = 1.66 x 10^(-18) moles x 74.14 g/mol = 1.23 x 10^(-16) g. The mass of 1.0 x 10^6 molecules of dimethylnitrosamine is 1.23 x 10^(-16) g. #f. Calculate the mass in grams of one molecule of dimethylnitrosamine#
10

Calculate moles from number of molecules

To calculate moles for one molecule, use Avogadro's number: Moles = 1 molecule / \(6.022 \times 10^{23}\) molecules/mol = 1.66 x 10^(-24) moles.
11

Calculate mass from moles and molar mass

To calculate the mass: Mass = (Moles) x (Molar mass) = 1.66 x 10^(-24) moles x 74.14 g/mol = 1.23 x 10^(-22) g. The mass of one molecule of dimethylnitrosamine is 1.23 x 10^(-22) g.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding the Mole Concept
To fully grasp chemistry, it's essential to understand the mole concept, which is a fundamental unit in chemistry representing a specific number of particles, atoms, or molecules. Essentially, the mole is a bridge between the microscopic world of atoms and molecules and the macroscopic world of grams and liters that we can measure in the lab.

The mole concept is integral for quantifying substances in chemical reactions. One mole of any substance contains exactly the same number of particles as there are atoms in exactly 12 grams of carbon-12. This number is Avogadro's number, which is approximately \(6.022 \times 10^{23}\).

When asked about the mass of moles or the number of particles in a substance, you'll be using the mole concept to convert between mass, moles, and particle count. In the textbook exercise, for example, you calculated the number of moles in a given mass of dimethylnitrosamine (\

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Silver sulfadiazine burn-treating cream creates a barrier against bacterial invasion and releases antimicrobial agents directly into the wound. If \(25.0 \mathrm{~g} \mathrm{Ag}_{2} \mathrm{O}\) is reacted with \(50.0 \mathrm{~g} \mathrm{C}_{10} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{SO}_{2}\), what mass of silver sulfadiazine, \(\mathrm{AgC}_{10} \mathrm{H}_{9} \mathrm{~N}_{4} \mathrm{SO}_{2}\), can be produced, assuming \(100 \%\) yield? \(\mathrm{Ag}_{2} \mathrm{O}(s)+2 \mathrm{C}_{10} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{SO}_{2}(s) \longrightarrow 2 \mathrm{AgC}_{10} \mathrm{H}_{9} \mathrm{~N}_{4} \mathrm{SO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l)\)

Aspartame is an artificial sweetener that is 160 times sweeter than sucrose (table sugar) when dissolved in water. It is marketed as Nutra-Sweet. The molecular formula of aspartame is \(\mathrm{C}_{14} \mathrm{H}_{18} \mathrm{~N}_{2} \mathrm{O}_{5}\) a. Calculate the molar mass of aspartame. b. What amount (moles) of molecules are present in \(10.0 \mathrm{~g}\) aspartame? c. Calculate the mass in grams of \(1.56\) mol aspartame. d. What number of molecules are in \(5.0 \mathrm{mg}\) aspartame? e. What number of atoms of nitrogen are in \(1.2 \mathrm{~g}\) aspartame? f. What is the mass in grams of \(1.0 \times 10^{9}\) molecules of aspartame? g. What is the mass in grams of one molecule of aspartame?

When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture of \(\mathrm{FeO}\) and \(\mathrm{Fe}_{2} \mathrm{O}_{3} .\) In a certain experiment, \(20.00 \mathrm{~g}\) iron metal was reacted with \(11.20 \mathrm{~g}\) oxygen gas. After the experiment, the iron was totally consumed, and \(3.24 \mathrm{~g}\) oxygen gas remained. Calculate the amounts of \(\mathrm{FeO}\) and \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) formed in this experiment.

Boron consists of two isotopes, \({ }^{10} \mathrm{~B}\) and \({ }^{11} \mathrm{~B}\). Chlorine also has two isotopes, \({ }^{35} \mathrm{Cl}\) and \({ }^{37} \mathrm{Cl}\). Consider the mass spectrum of \(\mathrm{BCl}_{3}\). How many peaks would be present, and what approximate mass would each peak correspond to in the \(\mathrm{BCl}_{3}\) mass spectrum?

Bauxite, the principal ore used in the production of aluminum, has a molecular formula of \(\mathrm{Al}_{2} \mathrm{O}_{3}=2 \mathrm{H}_{2} \mathrm{O}\). a. What is the molar mass of bauxite? b. What is the mass of aluminum in \(0.58\) mol bauxite? c. How many atoms of aluminum are in \(0.58 \mathrm{~mol}\) bauxite? d. What is the mass of \(2.1 \times 10^{24}\) formula units of bauxite?
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.