Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 42

What number of Fe atoms and what amount (moles) of Fe atoms are in \(500.0 \mathrm{~g}\) of iron?

Short Answer

Expert verified
In 500.0 g of iron, there are 8.951 moles of Fe atoms and 5.385 × 10^24 Fe atoms.

Step by step solution

01

Calculate moles of Fe in 500 grams

To calculate the amount of iron (Fe) in moles, we need to divide the given mass (500 grams) by the molar mass of iron (55.845 g/mol). Using the formula: Moles of Fe = (mass of Fe) / (molar mass of Fe) Moles of Fe = \( \frac{500.0}{55.845} \)
02

Perform the division

Now we simply perform the division operation to get the amount (moles) of Fe atoms: Moles of Fe = 8.951 moles (rounded to three decimal places)
03

Calculate the number of Fe atoms

We know that 1 mole consists of Avogadro's number (6.022 × 10^23 atoms/mol) of atoms. To calculate the number of Fe atoms in 8.951 moles, we simply multiply the moles by Avogadro's number: Fe atoms = (moles of Fe) × (Avogadro's number) Fe atoms = (8.951 moles) × (6.022 × 10^23 atoms/mol)
04

Perform the multiplication

Now, we perform the multiplication to get the total number of Fe atoms: Fe atoms = 5.385 × 10^24 atoms (rounded to three decimal places) So, there are 5.385 × 10^24 Fe atoms and 8.951 moles of Fe atoms in 500.0 g of iron.

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

A given sample of a xenon fluoride compound contains molecules of the type \(\mathrm{XeF}_{n}\), where \(n\) is some whole number. Given that \(9.03 \times 10^{20}\) molecules of \(\mathrm{XeF}_{n}\) weigh \(0.368 \mathrm{~g}\), determine the value for \(n\) in the formula.

A binary compound between an unknown element \(\mathrm{E}\) and hydrogen contains \(91.27 \% \mathrm{E}\) and \(8.73 \% \mathrm{H}\) by mass. If the formula of the compound is \(\mathrm{E}_{3} \mathrm{H}_{\mathrm{s}}\), calculate the atomic mass of \(\mathrm{E}\).

Give the balanced equation for each of the following chemical reactions: a. Glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{t}\right)\) reacts with oxygen gas to produce gaseous carbon dioxide and water vapor. b. Solid iron(III) sulfide reacts with gaseous hydrogen chloride to form solid iron(III) chloride and hydrogen sulfide gas. c. Carbon disulfide liquid reacts with ammonia gas to produce hydrogen sulfide gas and solid ammonium thiocyanate \(\left(\mathrm{NH}_{4} \mathrm{SCN}\right)\).

DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: $$ 2 \mathrm{C}_{6} \mathrm{H}_{3} \mathrm{Cl}+\mathrm{C}_{2} \mathrm{HOCl}_{3} \longrightarrow \mathrm{C}_{14} \mathrm{H}_{4} \mathrm{Cl}_{5}+\mathrm{H}_{2} \mathrm{O} $$ \(\begin{array}{ll}\text { orobenzenc chloral } & \mathrm{D}\end{array}\) In a government lab, \(1142 \mathrm{~g}\) of chlorobenzene is reacted with \(485 \mathrm{~g}\) of chloral. a. What mass of DDT is formed? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is \(200.0 \mathrm{~g}\), what is the percent yield?

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?
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Kinetics

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