Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 41

A compound \(\mathrm{XCl}_{3}\) is \(70.3 \%\) (by mass) chlorine. What is the molar mass of the compound? What is the symbol and name of X?

Short Answer

Expert verified
Question: Given a compound XCl3, where chlorine makes up 70.3% of the mass, find the molar mass of the compound and identify the element X. Answer: To calculate the molar mass of the compound XCl3, first determine the mass of the three chlorine atoms and the unknown element X. Then, add the molar mass of X to the molar mass of three chlorine atoms. Finally, identify the unknown element X based on its molar mass found in the periodic table.

Step by step solution

01

Determine the mass of chlorine in the compound

If chlorine makes up 70.3% of the mass of the compound XCl3, then we can find the mass of chlorine as: Mass of chlorine (g) = (\(70.3 \times \mathrm{mass\, of\, the\, compound\,} (g))/100\)
02

Determine the mass of the unknown element X

Using the percentage mass of chlorine, we can find the percentage mass of the unknown element X as 100% - 70.3% = 29.7%. Thus, the mass of the unknown element X (g) can be calculated as follows: Mass of X (g) = (\(29.7 \times \mathrm{mass\, of\, the\, compound\,} (g))/100\)
03

Determine the molar mass of the compound XCl3

We know that there are three chlorine atoms in the compound XCl3. The molar mass of one chlorine atom is 35.45 g/mol. Therefore, the molar mass of three chlorine atoms is: \(3 \times 35.45\,\mathrm{g/mol} = 106.35\,\mathrm{g/mol}\) Next, we will use the mass of the unknown element X we found in step 2 and divide it by the molar mass of the three chlorine atoms: Molar mass of X = (Mass of X (g))/(106.35 g/mol)
04

Identify element X based on its molar mass

Once we have calculated the molar mass of the unknown element X, we can use the periodic table to identify the element based on its atomic mass. For example, if the molar mass of X is close to 118.71 g/mol, then the element X is tin (Sn).
05

Calculate the molar mass of the compound XCl3

Now that we have identified the unknown element X, we can calculate the molar mass of the compound XCl3 by adding the molar mass of X to the molar mass of the three chlorine atoms: Molar mass of XCl3 = Molar mass of X + Molar mass of 3 Cl

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

97\. Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required) in the blanks provided. (a) The mass (to three significant figures) of \(6.022 \times 10^{23}\) atoms of Na ______ 23.0 g. (b) Boron has two isotopes, B-10 (10.01 amu) and B-11 (11.01 amu). The abundance of B-10 _______the abundance of B-11. (c) If S-32 were assigned as the standard for expressing relative atomic masses and assigned an atomic mass of \(10.00 \mathrm{amu}\), the atomic mass for \(\mathrm{H}\) would be _____\(1.00 \mathrm{amu} .\) (d) When phosphine gas, \(\mathrm{PH}_{3}\), is burned in oxygen, tetraphosphorus decaoxide and steam are formed. In the balanced equation (using smallest whole-number coefficients) for the reaction, the sum of the coefficients on the reactant side is _______ \(7 .\) (e) The mass (in grams) of one mole of bromine molecules is _______ \(79.90\)

Riboflavin is one of the \(\mathrm{B}\) vitamins. It is also known as vitamin \(\mathrm{B}_{6}\) and is made up of carbon, hydrogen, nitrogen, and oxygen atoms. When \(10.00 \mathrm{~g}\) of vitamin \(\mathrm{B}_{6}\) is burned in oxygen, \(19.88 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) and \(4.79 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\) are obtained. Another experiment shows that vitamin \(\mathrm{B}_{6}\) is made up of \(14.89 \% \mathrm{~N}\). What is the simplest formula for vitamin \(\mathrm{B}_{6}\) ?

Suppose that the atomic mass of \(\mathrm{C}-12\) is taken to be \(5.000 \mathrm{amu}\) and that a mole is defined as the number of atoms in \(5.000 \mathrm{~kg}\) of carbon-12. How many atoms would there be in one mole under these conditions? (Hint: There are \(6.022 \times 10^{23} \mathrm{C}\) atoms in \(12.00 \mathrm{~g}\) of \(\mathrm{C}-12 .\) )

Ibuprofen, the active ingredient in Advil \(^{\text {m }}\), is made up of carbon, hydrogen, and oxygen atoms. When a sample of ibuprofen, weighing \(5.000 \mathrm{~g}\), burns in oxygen, \(13.86 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) and \(3.926 \mathrm{~g}\) of water are obtaine \(\mathrm{d} .\) What is the simplest formula of ibuprofen?

A certain hydrate of potassium aluminum sulfate (alum) has the formula \(\mathrm{KAl}\left(\mathrm{SO}_{4}\right)_{2} \cdot x \mathrm{H}_{2} \mathrm{O}\). When a hydrate sample weighing \(5.459 \mathrm{~g}\) is heated to remove all the water, \(2.583 \mathrm{~g}\) of \(\mathrm{KAl}\left(\mathrm{SO}_{4}\right)_{2}\) remains. What is the mass percent of water in the hydrate? What is \(x ?\)
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation

Kinetics

Read Explanation

Organic Chemistry

Read Explanation

Making Measurements

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