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Chapter 3: Problem 63

Convert the following into balanced equations: (a) When lead(II) nitrate solution is added to potassium iodide solution, solid lead(II) iodide forms and potassium nitrate solution remains. (b) Liquid disilicon hexachloride reacts with water to form solid silicon dioxide, hydrogen chloride gas, and hydrogen gas. (c) When nitrogen dioxide is bubbled into water, a solution of nitric acid forms and gaseous nitrogen monoxide is released.

Short Answer

Expert verified
(a) 2 KI + Pb(NO₃)₂ → PbI₂ + 2 KNO₃ (b) Si₂Cl₆ + 3 H₂O → 2 SiO₂ + 6 HCl + 2 H₂ (c) 3 NO₂ + H₂O → 2 HNO₃ + NO

Step by step solution

01

Write the Unbalanced Equation for Reaction (a)

Begin by writing the reactants and products for the first reaction. Lead(II) nitrate (Pb(NO₃)₂) reacts with potassium iodide (KI) to form lead(II) iodide (PbI₂) and potassium nitrate (KNO₃). The unbalanced equation is: Pb(NO₃)₂ (aq) + KI (aq) → PbI₂ (s) + KNO₃ (aq)
02

Balance the Equation for Reaction (a)

Next, balance the equation by adjusting the coefficients. 2 KI (aq) + Pb(NO₃)₂ (aq) → PbI₂ (s) + 2 KNO₃ (aq)
03

Write the Unbalanced Equation for Reaction (b)

Write the reactants and products for the second reaction. Disilicon hexachloride (Si₂Cl₆) reacts with water (H₂O) to form silicon dioxide (SiO₂), hydrogen chloride (HCl), and hydrogen gas (H₂). The unbalanced equation is: Si₂Cl₆ (l) + H₂O (l) → SiO₂ (s) + HCl (g) + H₂ (g)
04

Balance the Equation for Reaction (b)

Now, balance the equation. Si₂Cl₆ (l) + 3 H₂O (l) → 2 SiO₂ (s) + 6 HCl (g) + 2 H₂ (g)
05

Write the Unbalanced Equation for Reaction (c)

Write the reactants and products for the third reaction. Nitrogen dioxide (NO₂) reacts with water (H₂O) to form nitric acid (HNO₃) and nitrogen monoxide (NO). The unbalanced equation is: NO₂ (g) + H₂O (l) → HNO₃ (aq) + NO (g)
06

Balance the Equation for Reaction (c)

Finally, balance the equation. 3 NO₂ (g) + H₂O (l) → 2 HNO₃ (aq) + NO (g)

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It helps us predict the amounts of substances consumed and produced. When balancing equations, stoichiometry ensures that the amount of each element is conserved. This is crucial because we need the same number of atoms of each element on both sides of the equation. Using stoichiometry, we can calculate the exact ratios of reactants needed to yield a specific amount of product.
Chemical Reactions
Chemical reactions involve the transformation of reactants into products. In a reaction, the chemical bonds of the reactants are broken, and new bonds are formed to create the products. Each reaction can be represented by a chemical equation, which shows the reactants on the left and the products on the right. Understanding chemical reactions includes knowing the types of reactions, such as synthesis, decomposition, single replacement, and double replacement. Each type of reaction follows specific patterns and rules. For example, in a double replacement reaction like in part (a) of the exercise, ions in two compounds exchange places to form two new compounds.
Molecular Equations
Molecular equations provide a way to represent chemical reactions by showing the complete formulas of the compounds involved, without breaking them down into ions. In our example, the molecular equations are written before balancing them, like: Pb(NO₃)₂ (aq) + KI (aq) → PbI₂ (s) + KNO₃ (aq). These equations help visualize the reactants transforming into products. However, to fully understand the reaction, balancing the equation is necessary. Only then does the equation accurately represent the conservation of mass and moles.
Reactants and Products
Reactants are the starting substances in a chemical reaction, and products are the substances formed as a result. For illustration, in reaction (a), the reactants are lead(II) nitrate and potassium iodide, while the products are lead(II) iodide and potassium nitrate. Identifying reactants and products is the first step in writing a chemical equation. Knowing how reactants interact helps us predict the products. Each reaction must be balanced to ensure that the same amount of matter exists before and after the reaction, aligning with the law of conservation of mass.
Law of Conservation of Mass
The law of conservation of mass states that mass cannot be created or destroyed in a chemical reaction. This principle requires that the mass of the reactants equal the mass of the products. When balancing chemical equations, we apply this law by ensuring that the number of each type of atom on the reactant side matches the number on the product side. Take, for example, reaction (b): Si₂Cl₆ (l) + 3 H₂O (l) → 2 SiO₂ (s) + 6 HCl (g) + 2 H₂ (g). Initially, the equation may not follow this law, but adjusting the coefficients ensures that it does. This balance verifies that the reaction aligns with the conservation of mass.

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Most popular questions from this chapter

Aspirin (acetylsalicylic acid, \(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\) ) is made by reacting salicylic acid \(\left(\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}\right)\) with acetic anhydride \(\left[\left(\mathrm{CH}_{3} \mathrm{CO}\right)_{2} \mathrm{O}\right]:\) $$ \mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}(s)+\left(\mathrm{CH}_{3} \mathrm{CO}\right)_{2} \mathrm{O}(l) \longrightarrow \mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}(s)+\mathrm{CH}_{3} \mathrm{COOH}(l) $$ In one preparation, \(3.077 \mathrm{~g}\) of salicylic acid and \(5.50 \mathrm{~mL}\) of acetic anhydride react to form \(3.281 \mathrm{~g}\) of aspirin. (a) Which is the limiting reactant (the density of acetic anhydride is \(1.080 \mathrm{~g} / \mathrm{mL}) ?\) (b) What is the percent yield of this reaction? (c) What is the percent atom economy of this reaction?

Is each of the following statements true or false? Correct any that are false. (a) A mole of one substance has the same number of atoms as a mole of any other substance. (b) The theoretical yield for a reaction is based on the balanced chemical equation. (c) A limiting-reactant problem is being stated when the available quantity of one of the reactants is given in moles. (d) The empirical and molecular formulas of a compound are always different.

What are the empirical formula and empirical formula mass for each of the following compounds? (a) \(\mathrm{C}_{2} \mathrm{H}_{4}\) (b) \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\) (c) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (d) \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) (e) \(\mathrm{Te}_{4} \mathrm{I}_{16}\)

Serotonin \((\mathscr{M}=176 \mathrm{~g} / \mathrm{mol})\) transmits nerve impulses between neurons. It contains \(68.2 \%\) C, \(6.86 \%\) H, \(15.9 \%\) N, and \(9.08 \%\) O by mass. What is its molecular formula?

Lead can be prepared from galena [lead(II) sulfide] by first roasting the galena in oxygen gas to form lead(II) oxide and sulfur dioxide. Heating the metal oxide with more galena forms the molten metal and more sulfur dioxide. (a) Write a balanced equation for each step. (b) Write an overall balanced equation for the process. (c) How many metric tons of sulfur dioxide form for every metric ton of lead obtained?
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