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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 quantity of a reactant because it ensures the Law of Conservation of Mass is obeyed and provides stoichiometric coefficients for stoichiometry calculations. These coefficients help in accurately predicting reactant amounts required and product amounts formed, allowing for efficient planning and optimization of chemical reactions while reducing waste.

Step by step solution

01

Balanced Chemical Equations

In a balanced chemical equation, the number of atoms of each element is the same on the reactant side and the product side. This ensures that the Law of Conservation of Mass is followed, meaning the total mass of reactants is equal to the total mass of products. A balanced chemical equation also represents the stoichiometric coefficients, showing the relationship between moles of reactants and products.
02

Stoichiometry

Stoichiometry is the calculation of the quantities of reactants and products in a chemical reaction. It is based on the coefficients of the balanced chemical equation, which provide the molar proportions of the substances involved. These coefficients help us in determining the mass of reactants needed to produce a desired mass of products or to calculate the mass of products formed from a given mass of reactants.
03

Importance of Balanced Chemical Equations

When determining the quantity of a product formed from a given quantity of a reactant, it's essential to use a balanced chemical equation because: 1. It obeys the Law of Conservation of Mass, ensuring that the mass of reactants equals the mass of products. 2. It provides stoichiometric coefficients, which are crucial for carrying out stoichiometry calculations. 3. It helps predict the reactant amounts required to produce a desired quantity of products, as well as the product amounts formed from given quantities of reactant. 4. It allows for efficient planning and optimization of chemical reactions, as well as reducing waste by accurately calculating the required amounts of reactants. By using balanced chemical equations, we ensure the accuracy of our calculations related to chemical reactions and their material quantifications, making it essential for determining the quantity of a product formed from a given quantity of a reactant.

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Most popular questions from this chapter

Aluminum hydroxide reacts with sulfuric acid as follows: \(2 \mathrm{Al}(\mathrm{OH})_{3}(s)+3 \mathrm{H}_{2} \mathrm{SO}_{4}(a q)\) \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l)\) Which reagent is the limiting reactant when \(0.500 \mathrm{~mol}\) \(\mathrm{Al}(\mathrm{OH})_{3}\) and \(0.500 \mathrm{~mol} \mathrm{H}_{2} \mathrm{SO}_{4}\) are allowed to react? How many moles of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) can form under these conditions? How many moles of the excess reactant remain after the completion of the reaction?

(a) What is the difference between adding a subscript 2 to the end of the formula for CO to give \(\mathrm{CO}_{2}\) and adding a coefficient in front of the formula to give \(2 \mathrm{CO}\) ? (b) Is the following chemical equation, as written, consistent with the law of conservation of mass? \(3 \mathrm{Mg}(\mathrm{OH})_{2}(s)+2 \mathrm{H}_{3} \mathrm{PO}_{4}(a q) \longrightarrow \mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}(5)+6 \mathrm{H}_{2} \mathrm{O}(l)\) Why or why not?

Determine the empirical formula of each of the following compounds if a sample contains (a) \(0.104 \mathrm{~mol} \mathrm{~K}\). \(0.052 \mathrm{~mol} \mathrm{C}\), and \(0.156 \mathrm{~mol} \mathrm{O} ;\) (b) \(5.28 \mathrm{~g} \mathrm{Sn}\) and \(3.37 \mathrm{~g} \mathrm{~F}\); (c) \(87.5 \% \mathrm{~N}\) and \(12.5 \% \mathrm{H}\) by mass.

A chemical plant uses electrical energy to decompose aqueous solutions of \(\mathrm{NaCl}\) to give \(\mathrm{Cl}_{2}, \mathrm{H}_{2}\), and \(\mathrm{NaOH}\) : \(2 \mathrm{NaCl}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \underset{2 \mathrm{NaOH}(a q)}{\longrightarrow}+\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g)\) If the plant produces \(1.5 \times 10^{6} \mathrm{~kg}\left(1500\right.\) metric tons) of \(\mathrm{Cl}_{2}\) daily, estimate the quantities of \(\mathrm{H}_{2}\) and \(\mathrm{NaOH}\) produced.

The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet \(^{0}\), is \(\mathrm{C}_{14} \mathrm{H}_{18} \mathrm{~N}_{2} \mathrm{O}_{5}\) (a) What is the molar mass of aspartame? (b) How many moles of aspartame are present in \(1.00 \mathrm{mg}\) of aspartame? (c) How many molecules of aspartame are present in \(1.00 \mathrm{mg}\) of aspartame? (d) How many hydrogen atoms are present in \(1.00 \mathrm{mg}\) of aspartame?
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