Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 28

How many grams are present in \(4.336 \times 10^{24}\) formula units of table salt, NaCl, whose molar mass is 58.44 \(\mathrm{g} / \mathrm{mol} ?\)

Short Answer

Expert verified
To find the final answer, complete the calculations in steps 1 and 2. The answer will be in grams.

Step by step solution

01

Calculate number of moles

The molar mass of NaCl is given as 58.44 g/mol. However, we are given the quantity of formula units, not grams or moles, so our first step will be converting formula units to moles. Using Avogadro's number \(6.022 \times 10^{23} \) formula units/mol, we can find moles from the formula units. Using the formula: \[ moles = \frac{formula~units}{Avogadro's~number} = \frac{4.336 \times 10^{24}}{6.022 \times 10^{23}} \]
02

Convert moles to grams

Now that we have the number of moles, we can convert this to grams using the molar mass of NaCl which is given as 58.44 g/mol. Thus, \[ grams = moles \times molar~mass = moles \times 58.44 \]
03

Calculate and Present the Final Answer

Perform the multiplication found in step 2 to get the final answer.

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

How many molecules in 2.00 \(\mathrm{mol}\) of sucrose, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11} ?\)

What is the molar mass of the amino acid glycine, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2} ?\)

How many atoms are in the \(1.25 \times 10^{-2}\) mol of mercury within the bulb of a thermometer?

The empirical formula of the anticancer drug altretamine is \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{N}_{2}\) . The experimental molar mass is 210 \(\mathrm{g} / \mathrm{mol} .\) What is its molecular formula?

Calculate the mass of each of the following samples: a. 0.500 \(\mathrm{mol} \mathrm{I}_{2}\) (molar mass of \(\mathrm{I}_{2}=\) 253.80 \(\mathrm{g} / \mathrm{mol} )\) b. 2.82 mol PbS (molar mass of PbS = 239.3 g/mol) c.4 .00 \(\mathrm{mol}\) of \(\mathrm{C}_{4} \mathrm{H}_{10}\) (molar mass of \(\mathrm{C}_{4} \mathrm{H}_{10}=\) 58.14 \(\mathrm{g} / \mathrm{mol} )\)
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear 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