Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 32

The food flavor enhancer monosodium glutamate (MSG) has the composition \(13.6 \%\) Na, \(35.5 \%\) C. \(4.8 \% \mathrm{H}, 8.3 \% \mathrm{N}, 37.8 \% \mathrm{O},\) by mass. What is the empirical formula of MSG?

Short Answer

Expert verified
The empirical formula of Monosodium Glutamate (MSG) is \( NaC_5H_8N_1O_4 \).

Step by step solution

01

Convert Percentages to Moles

First, treat the percentages as grams (since percentages are parts per hundred) and convert these to moles. Here's how you convert for each element: For \( Na \), given is 13.6 %. So the moles of \( Na \) will be: \( \frac{13.6}{23.0} = 0.59 \). Similarly, Calculate the moles for all the other elements: \( C = \frac{35.5}{12.01} = 2.96 \), \( H = \frac{4.8}{1.01} = 4.75 \), \( N = \frac{8.3}{14.01} = 0.59 \), and \( O = \frac{37.8}{16.0} = 2.36 \).
02

Finding the Simplest Ratio

Now you have to find the simplest whole number ratio of these moles. Divide each value by the smallest number of moles calculated in the previous step. So the smallest number of moles in this calculation is 0.59. We divide all the values by 0.59. The result is: \( Na = 1 \), \( C = 5 \), \( H = 8 \), \( N = 1 \), \( O = 4 \). These are the simplest ratios in integers for each element in MSG.
03

Writing the Empirical Formula

The empirical formula is written by arranging the elements together with their simplest ratios. As per the ratios arrived at in the last step, the empirical formula of Monosodium Glutamate (MSG) is: \( NaC_5H_8N_1O_4 \).

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

Three of the following formulas might be either an empirical or a molecular formula. The formula that must be a molecular formula is (a) \(\mathrm{N}_{2} \mathrm{O} ;\) (b) \(\mathrm{N}_{2} \mathrm{H}_{4}\) (c) \(\mathrm{NaCl} ;\) (d) \(\mathrm{NH}_{3}\)

An 8.129 g sample of \(\mathrm{MgSO}_{4} \cdot x \mathrm{H}_{2} \mathrm{O}\) is heated until all the water of hydration is driven off. The resulting anhydrous compound, \(\mathrm{MgSO}_{4},\) weighs \(3.967 \mathrm{g} .\) What is the formula of the hydrate?

Name the following compounds and specify which ones are best described as ionic: (a) \(\mathrm{KNO}_{2} ;\) (b) \(\mathrm{Br} \mathrm{F}_{3}\) (c) \(\mathrm{S}_{2} \mathrm{Cl}_{2} ;\) (d) \(\mathrm{Mg}(\mathrm{ClO})_{2} ;\) (e) \(\mathrm{Cl}_{2} \mathrm{O}\)

Two compounds of \(\mathrm{Cl}\) and \(\mathrm{X}\) are found to have molecular masses and \% Cl, by mass, as follows: 137 u, \(77.5 \% \mathrm{Cl} ; 208 \mathrm{u}, 85.1 \%\) Cl. What is element \(\mathrm{X} ?\) What is the formula for each compound?

Selenium, an element used in the manufacture of photoelectric cells and solar energy devices, forms two oxides. One has \(28.8 \%\) O, by mass, and the other, 37.8\% O. What are the formulas of these oxides? Propose acceptable names for them.
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

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