/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 55 Why is it essential to use balan... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 3: Problem 55

Why is it essential to use balanced chemical equations when determining the quantity of a product formed from a given quantity of a reactant?

Short Answer

Expert verified
Using balanced chemical equations is essential when determining the quantity of a product formed from a given reactant because it ensures compliance with the law of conservation of mass and allows for accurate predictions based on stoichiometry. The balanced equation provides the correct mole ratio between reactants and products, enabling chemists to determine the correct proportions and avoid inaccurate, incomplete, or wasteful reactions. Without a balanced equation, it would be impossible to accurately predict product quantities or determine the efficiency of a chemical reaction.

Step by step solution

01

Importance of Balanced Chemical Equations

Balancing a chemical equation is essential because it ensures that the law of conservation of mass is upheld, meaning the total mass of reactants equals the total mass of products. Balanced chemical equations express the relationship between substances participating in a chemical reaction and indicate the correct amounts of each reactant and product in the reaction.
02

Stoichiometry and Conservation of Mass

Stoichiometry is the quantitative relationship between the amounts of reactants and products in a balanced chemical equation. The coefficients in a balanced equation indicate the mole ratio between different reactants and products. This mole ratio allows us to calculate the quantity of one substance (product or reactant) required or produced, given the initial quantity of another substance.
03

Determining Product Quantity

Using balanced chemical equations is essential when determining the quantity of a product formed from a given reactant because it allows for accurate predictions based on the stoichiometric relationships. Without a balanced equation, it would be impossible to know the correct proportions of reactants needed to produce the desired product without waste or excess reactants, leading to inaccurate, incomplete, or inefficient reactions. For example, consider the following balanced equation for the reaction between hydrogen gas and oxygen gas to form water: \(2 H_2 + O_2 \rightarrow 2 H_2O\) Here, 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water. If we're given the quantity of hydrogen gas and asked how much water is produced, we can use stoichiometry to calculate the answer based on the balanced equation. If the equation were not balanced, we would not know the correct mole ratio between hydrogen, oxygen, and water, making it impossible to determine the product quantities accurately.
04

Conclusion

Balanced chemical equations are essential when determining the quantity of a product formed from a given reactant to ensure compliance with the law of conservation of mass. This allows for accurate predictions based on stoichiometry and enables chemists to determine the correct proportions of reactants and products in a chemical reaction. Inaccurate or unbalanced equations would lead to incorrect, incomplete, or wasteful reactions, making it impossible to accurately predict product quantities or determine the efficiency of a chemical reaction.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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

The koala dines exclusively on eucalyptus leaves. Its digestive system detoxifies the eucalyptus oil, a poison to other animals. The chief constituent in eucalyptus oil is a substance called eucalyptol, which contains \(77.87 \% \mathrm{C}\), \(11.76 \% \mathrm{H}\), and the remainder \(\mathrm{O}\). (a) What is the empirical formula for this substance? (b) A mass spectrum of eucalyptol shows a peak at about 154 amu. What is the molecular formula of the substance?

Balance the following equations: (a) \(\mathrm{Li}(s)+\mathrm{N}_{2}(g) \longrightarrow \mathrm{Li}_{3} \mathrm{~N}(s)\) (b) \(\mathrm{La}_{2} \mathrm{O}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{La}(\mathrm{OH})_{3}(a q)\) (c) \(\mathrm{NH}_{4} \mathrm{NO}_{3}(s) \longrightarrow \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) (d) \(\mathrm{Ca}_{3} \mathrm{P}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{PH}_{3}(g)\) (e) \(\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{3} \mathrm{PO}_{4}(a q) \longrightarrow\) \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l)\) (f) \(\mathrm{AgNO}_{3}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\) \(\mathrm{Ag}_{2} \mathrm{SO}_{4}(\mathrm{~s})+\mathrm{NaNO}_{3}(a q)\) (g) \(\mathrm{CH}_{3} \mathrm{NH}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow\) \(\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{N}_{2}(g)\)

The molecular formula of allicin, the compound responsible for the characteristic smell of garlic, is \(\mathrm{C}_{6} \mathrm{H}_{10} \mathrm{OS}_{2}\). (a) What is the molar mass of allicin? (b) How many moles of allicin are present in \(5.00 \mathrm{mg}\) of this substance? (c) How many molecules of allicin are in \(5.00 \mathrm{mg}\) of this substance? (d) How many \(\mathrm{S}\) atoms are present in 5.00 mg of allicin?

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of \(\mathrm{NH}_{3}\) to \(\mathrm{NO}\) : $$ 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) $$ In a certain experiment, \(1.50 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) reacts with \(2.75 \mathrm{~g}\) of \(\mathrm{O}_{2}\) (a) Which is the limiting reactant? (b) How many grams of \(\mathrm{NO}\) and of \(\mathrm{H}_{2} \mathrm{O}\) form? (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed? (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

Calculate the following quantities: (a) mass, in grams, of \(0.105\) moles sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) (b) moles of \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}\) in \(143.50 \mathrm{~g}\) of this substance (c) number of molecules in \(1.0 \times 10^{-6} \mathrm{~mol} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) (d) number of \(\mathrm{N}\) atoms in \(0.410 \mathrm{~mol} \mathrm{NH}_{3}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

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.