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Chapter 3: Problem 61

On what law is stoichiometry based? Why is it essential to use balanced equations in solving stoichiometric problems?

Short Answer

Expert verified
Stoichiometry is based on the Law of Conservation of Mass, which states that the mass of the reactants must equal the mass of the products in a chemical reaction. Balanced equations are essential in stoichiometry as they align with this law, indicating the quantity of reactants required or the quantity of products formed during a chemical reaction.

Step by step solution

01

Understanding Stoichiometry

Stoichiometry is a branch of chemistry that deals with the quantitative relationships that exist among the reactants and products in chemical reactions.
02

Law Governing Stoichiometry

Stoichiometry is based on the Law of Conservation of Mass. This law states that matter cannot be created or destroyed. In a chemical reaction, the total mass of the reactants is equal to the total mass of the products.
03

Importance of Balanced Equations

Balanced equations are essential in stoichiometry as they reflect this Law of Conservation of Mass. They show how much reactants are needed or how much products are formed during a chemical reaction. Each coefficient in a balanced equation can be viewed as moles, allowing us to convert from moles of one substance to moles of another. This is key in solving stoichiometric problems.

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Most popular questions from this chapter

Calculate the molecular mass or formula mass (in amu) of each of the following substances: (a) \(\mathrm{CH}_{4}\) (b) \(\mathrm{NO}_{2},(\mathrm{c}) \mathrm{SO}_{3},\) (d) \(\mathrm{C}_{6} \mathrm{H}_{6}\) (e) NaI, (f) \(\mathrm{K}_{2} \mathrm{SO}_{4}\) \((\mathrm{g}) \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)

Hydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and in the production of aluminum metal. It is prepared by the reaction $$ \mathrm{CaF}_{2}+\mathrm{H}_{2} \mathrm{SO}_{4} \longrightarrow \mathrm{CaSO}_{4}+2 \mathrm{HF} $$ In one process \(6.00 \mathrm{~kg}\) of \(\mathrm{CaF}_{2}\) are treated with an excess of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and yield \(2.86 \mathrm{~kg}\) of \(\mathrm{HF}\). Calculate the percent yield of HF.

The molar mass of caffeine is \(194.19 \mathrm{~g}\). Is the molecular formula of caffeine \(\mathrm{C}_{4} \mathrm{H}_{5} \mathrm{~N}_{2} \mathrm{O}\) or \(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2} ?\)

For many years chloroform \(\left(\mathrm{CHCl}_{3}\right)\) was used as an inhalation anesthetic in spite of the fact that it is also a toxic substance that may cause severe liver, kidney, and heart damage. Calculate the percent composition by mass of this compound.

Use ammonia \(\left(\mathrm{NH}_{3}\right)\) to explain what is meant by the percent composition by mass of a compound.
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