Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 84

Carbon tetrachloride, \(\mathrm{CCl}_{4}\), was a popular dry-cleaning agent until it was shown to be carcinogenic. It has a density of \(1.589 \mathrm{~g} / \mathrm{cm}^{3} .\) What volume of carbon tetrachloride will contain a total of \(6.00 \times 10^{25}\) molecules of \(\mathrm{CCl}_{4} ?\)

Short Answer

Expert verified
Answer: The volume of carbon tetrachloride containing \(6.00 \times 10^{25}\) molecules of \(\mathrm{CCl}_{4}\) is \(9,646.90 \mathrm{cm^{3}}\).

Step by step solution

01

Find the molar mass of \(\mathrm{CCl}_{4}\)

First, determine the molar mass of carbon tetrachloride. Carbon has a molar mass of \(12.01 \mathrm{~g/mol}\) and Chlorine has a molar mass of \(35.45 \mathrm{~g/mol}\). So, the molar mass of \(\mathrm{CCl}_{4}\) is: \(1(12.01 \mathrm{~g/mol}) + 4(35.45 \mathrm{~g/mol}) = 12.01 + 4(35.45) = 12.01 + 141.8 = 153.81 \mathrm{~g/mol}\)
02

Determine the number of moles of \(\mathrm{CCl}_{4}\)

Next, we need to find the number of moles of \(\mathrm{CCl}_{4}\). We can use Avogadro's number (\(6.022 \times 10^{23} \mathrm{molecules/mol})\) to find the number of moles: Number of moles = (Number of molecules given) / (Avogadro's number) Number of moles = (\(6.00 \times 10^{25} \mathrm{molecules})\) / (\(6.022 \times 10^{23} \mathrm{molecules/mol}) = 99.63 \mathrm{mol}\)
03

Calculate the mass of \(\mathrm{CCl}_{4}\)

Now we will find the mass of carbon tetrachloride containing the given molecules. This can be found using the formula: Mass = (number of moles) × (molar mass) Mass = (99.63 \mathrm{mol}) × (153.81 \mathrm{~g/mol}) = 15,335.37 \mathrm{g}$
04

Calculate the volume of \(\mathrm{CCl}_{4}\)

Finally, we will use the density formula to find the volume of carbon tetrachloride containing the given molecules: Volume = (mass) / (density) Volume = \((15,335.37 \mathrm{g})\) / \((1.589 \mathrm{g/cm^{3}})\) = 9,646.90 \mathrm{cm^{3}}$ The volume of carbon tetrachloride containing \(6.00 \times 10^{25}\) molecules of \(\mathrm{CCl}_{4}\) is \(9,646.90 \mathrm{cm^{3}}\).

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

The meat from one hazelnut has a mass of \(0.985 \mathrm{~g}\). (a) What is the mass of a millionth of a mole \(\left(10^{-6}\right)\) of hazelnut meats? (A millionth of a mole is also called a micromole.) (b) How many moles are in a pound of hazelnut meats?

By \(x\) -ray diffraction it is possible to determine the geometric pattern in which atoms are arranged in a crystal and the distances between atoms. In a crystal of silver, four atoms effectively occupy the volume of a cube \(0.409 \mathrm{~nm}\) on an edge. Taking the density of silver to be \(10.5 \mathrm{~g} / \mathrm{cm}^{3}\), calculate the number of atoms in one mole of silver.

Nitrogen reacts with hydrogen to form ammonia. Represent each nitrogen atom by a square and each hydrogen atom with a circle. Starting with five molecules of both hydrogen and nitrogen, show pictorially what you have after the reaction is complete.

Deer ticks are known to cause Lyme disease. The presence of DEET (diethyltoluamide) in insect repellents protects the user from the ticks. The molecular formula for DEET is \(\mathrm{C}_{12} \mathrm{H}_{17} \mathrm{NO}\). How many grams of carbon can be obtained from \(127 \mathrm{~g}\) of DEET?

Write balanced equations for the reaction of sulfur with the following metals to form solids that you can take to be ionic when the anion is \(\mathrm{S}^{2-}\). (a) potassium (b) magnesium (c) aluminum (d) calcium (e) iron (forming \(\mathrm{Fe}^{2+}\) ions)
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Physical Chemistry

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.

Sign-up for free