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Chapter 9: Problem 18

What does it mean to say that the balanced chemical equation for a reaction describes the stoichiometry of the reaction?

Short Answer

Expert verified
A balanced chemical equation describes the stoichiometry of a reaction by providing quantitative relationships between reactants and products. It ensures that the number of atoms of each element on the reactant side is equal to the number on the product side, maintaining the law of conservation of mass. The coefficients in the balanced equation represent the molar ratios of reactants and products, allowing us to determine how much of each substance reacts and how much of each substance is produced during the reaction.

Step by step solution

01

Understanding stoichiometry

Stoichiometry refers to the quantitative relationship between reactants and products in a balanced chemical equation. It encompasses the study of how much of each reactant is consumed and how much of each product is formed during a chemical reaction.
02

Balanced chemical equation

A chemical equation is a representation of a chemical reaction, where reactants are written on the left side and products on the right side. The equation also provides information about the elemental composition and their relative quantities in a reaction. A balanced chemical equation ensures that the number of atoms of each element on the reactant side is equal to the number of atoms of that element on the product side, maintaining the law of conservation of mass.
03

Connecting stoichiometry and balanced chemical equation

A balanced chemical equation gives us the stoichiometry of a reaction. The coefficients in the balanced equation represent the molar ratios of the reactants and products, which help to determine how much of each substance reacts and how much of each substance is produced during the reaction. For instance, consider the balanced chemical equation for the reaction between hydrogen and oxygen to produce water: \[2H_2 + O_2 \rightarrow 2H_2O\] In this equation, the numbers in front of each molecule (called coefficients) represent the stoichiometric coefficients. According to the coefficients, two moles of hydrogen gas react with one mole of oxygen gas to produce two moles of water. So, when we say that the balanced chemical equation describes the stoichiometry of a reaction, it means that the equation provides us with the quantitative relationships between the reactants and products in a chemical reaction, allowing us to calculate how much of each substance is needed or produced.

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Most popular questions from this chapter

For each of the following reactions, give the balanced equation for the reaction and state the meaning of the equation in terms of the numbers of individual molecules and in terms of moles of molecules. a. \(\mathrm{PCl}_{3}(l)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{3}(a q)+\mathrm{HCl}(g)\) b. \(\mathrm{XeF}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{Xe}(g)+\mathrm{HF}(g)+\mathrm{O}_{2}(g)\) c. \(S(s)+H N O_{3}(a q) \rightarrow H_{2} S O_{4}(a q)+H_{2} O(l)+N O_{2}(g)\) d. \(\mathrm{NaHSO}_{3}(s) \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{3}(s)+\mathrm{SO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\)

Using the average atomic masses given inside the front cover of this book, calculate the mass in grams of each of the following samples. a. 4.25 mol of oxygen gas, \(\mathrm{O}_{2}\) b. 1.27 millimol of platinum (1 millimol \(=1 / 1000\) mol) c. 0.00101 mol of iron(II) sulfate, \(\mathrm{FeSO}_{4}\) d. 75.1 mol of calcium carbonate, \(\mathrm{CaCO}_{3}\) e. \(1.35 \times 10^{-4}\) mol of gold f. 1.29 mol of hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\) g. 6.14 mol of copper(II) sulfide, Cus

For each of the following incomplete and unbalanced equations, indicate how many moles of the second reactant would be required to react completely with 0.145 mol of the first reactant. a. \(\mathrm{BaCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow\) b. \(\operatorname{AgNO}_{3}(a q)+\operatorname{NaCl}(a q) \rightarrow\) c. \(\operatorname{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \rightarrow\) d. \(C_{3} \mathrm{H}_{8}(g)+\mathrm{O}_{2}(g) \rightarrow\)

For each of the following unbalanced chemical equations, suppose that exactly \(5.00 \mathrm{g}\) of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected (assuming that the limiting reactant is completely consumed). a. \(\mathrm{S}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{SO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) b. \(\operatorname{MnO}_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(l) \rightarrow \mathrm{Mn}\left(\mathrm{SO}_{4}\right)_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l)\) c. \(\mathrm{H}_{2} \mathrm{S}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{SO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) d. \(\mathrm{AgNO}_{3}(a q)+\mathrm{Al}(s) \rightarrow \mathrm{Ag}(s)+\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q)\)

For each of the following balanced chemical equations, calculate how many moles and how many grams of each product would be produced by the complete conversion of 0.50 mol of the reactant indicated in boldface. State clearly the mole ratio used for each conversion. a. \(\mathbf{N} \mathbf{H}_{3}(g)+\mathrm{HCl}(g) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(s)\) b. \(\mathrm{CH}_{4}(g)+\mathbf{4} \mathbf{S}(s) \rightarrow \mathrm{CS}_{2}(l)+2 \mathrm{H}_{2} \mathrm{S}(g)\) c. \(\mathbf{P C I}_{3}+3 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{3}(a q)+3 \mathrm{HCl}(a q)\) d. \(\mathbf{N a O H}(s)+\mathrm{CO}_{2}(g) \rightarrow \mathrm{NaHCO}_{3}(s)\)
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