Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 70

When baking soda (sodium bicarbonate or sodium hydrogen carbonate, \(\mathrm{NaHCO}_{3}\) ) is heated, it releases carbon dioxide gas, which is responsible for the rising of cookies, donuts, and bread. (a) Write a balanced equation for the decomposition of the compound (one of the products is \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) ). (b) Calculate the mass of \(\mathrm{NaHCO}_{3}\) required to produce \(20.5 \mathrm{~g}\) of \(\mathrm{CO}_{2.}\)

Short Answer

Expert verified
78.3g of NaHCO3 is required to produce 20.5g of CO2.

Step by step solution

01

Write the Balanced Chemical Equation

The decomposition of sodium bicarbonate upon heating results in the formation of sodium carbonate, water, and carbon dioxide. The balanced chemical equation for this is: \n\[2\mathrm{NaHCO}_{3}(s) \rightarrow \mathrm{Na}_{2}\mathrm{CO}_{3}(s) + \mathrm{H}_2\mathrm{O}(g) + \mathrm{CO}_2(g)\]
02

Calculate the Molar Mass of NaHCO3 and CO2

The molar mass of sodium bicarbonate (NaHCO3) is \(23.0 (Na) + 1.0 (H) + 12.0 (C) + 3 * 16.0 (O) = 84.0 \mathrm{~g/mol}\). Meanwhile, the molar mass of carbon dioxide (CO2) is \(12.0 (C) + 2 * 16.0 (O) = 44.0 \mathrm{~g/mol}\).
03

Apply Stoichiometry to Find Mass of NaHCO3 Needed

Using stoichiometry, you can establish molar ratios from the balanced chemical equation and then convert moles to mass. First, calculate the moles of CO2 produced from its given mass using its molar mass (\(20.5 \mathrm{~g} \div 44.0 \mathrm{~g/mol} = 0.466 \mathrm{~mol}\)). From the balanced equation, we can see that 2 moles of NaHCO3 will generate 1 mole of CO2. Therefore, the moles of NaHCO3 needed are \(2 * 0.466 \mathrm{~mol} = 0.932 \mathrm{~mol}\). Finally, multiply the moles of NaHCO3 by its molar mass to determine the mass needed (\(0.932 \mathrm{~mol} * 84.0 \mathrm{~g/mol} = 78.3 \mathrm{~g}\))
04

Conclusion

Therefore, to produce 20.5g of CO2, around 78.3g of NaHCO3 is required.

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 moles of calcium (Ca) atoms are in \(77.4 \mathrm{~g}\) of \(\mathrm{Ca} ?\)

What is the mass in grams of a single atom of each of the following elements? (a) As, (b) Ni.

The atomic masses of \({ }_{17}^{35} \mathrm{Cl}(75.53\) percent \()\) and \({ }_{17}^{37} \mathrm{Cl}\) (24.47 percent) are 34.968 amu and 36.956 amu, respectively. Calculate the average atomic mass of chlorine. The percentages in parentheses denote the relative abundances.

Calculate the molar mass of the following substances: (a) \(\mathrm{Li}_{2} \mathrm{CO}_{3},\) (b) \(\mathrm{CS}_{2},\) (c) \(\mathrm{CHCl}_{3}\) (chloroform), (d) \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{6}\) (ascorbic acid, or vitamin \(\mathrm{C}\) ), (e) \(\mathrm{KNO}_{3},\) (f) \(\mathrm{Mg}_{3} \mathrm{~N}_{2.}\)

Write the symbols used to represent gas, liquid, solid, and the aqueous phase in chemical equations.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Nuclear Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

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