Problem 45 Balance each of the following ch... [FREE SOLUTION]

Chapter 8: Problem 45

Balance each of the following chemical equations, and identify the type of reaction: \((8.1,8.2,8.3)\) a. \(\mathrm{NH}_{3}(g)+\mathrm{HCl}(g) \underset{\Delta}{\mathrm{NH}}_{4} \mathrm{Cl}(s)\) b. \(\mathrm{C}_{4} \mathrm{H}_{8}(g)+\mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) c. \(\mathrm{Sb}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{SbCl}_{3}(s)\) d. \(\mathrm{NI}_{3}(s) \longrightarrow \mathrm{N}_{2}(g)+\mathrm{I}_{2}(g)\) e. \(\mathrm{KBr}(a q)+\mathrm{Cl}_{2}(a q) \longrightarrow \mathrm{KCl}(a q)+\mathrm{Br}_{2}(I)\) f. \(\mathrm{Fe}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{H}_{2}(g)+\mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)\) g. \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+\mathrm{NaOH}(a q) \longrightarrow\) \(\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)\)

Short Answer

Expert verified

a) Combination, b) Combustion, c) Combination, d) Decomposition, e) Single replacement, f) Redox, g) Double displacement.

Step by step solution

Equation a: Initial Reaction

The given chemical equation is: \[\mathrm{NH}_3(g) + \mathrm{HCl}(g) \underset{\Delta}{\rightarrow} \mathrm{NH}_4\mathrm{Cl}(s)\]

Equation a: Balance the Equation

Count the number of atoms for each element on both sides of the equation. The number of N, H, and Cl atoms on both sides of the equation is already balanced (1 N, 4 H, 1 Cl).

Equation a: Identify Type of Reaction

This is a combination reaction because two reactants combine to form a single product.

Equation b: Initial Reaction

The given chemical equation is: \[\mathrm{C}_4\mathrm{H}_8(g) + \mathrm{O}_2(g) \underset{\Delta}{\rightarrow} \mathrm{CO}_2(g) + \mathrm{H}_2\mathrm{O}(g)\]

Equation b: Balance C and H Atoms

Balance the carbon and hydrogen atoms first: \[ \mathrm{C}_4\mathrm{H}_8(g) + \mathrm{O}_2(g) \underset{\Delta}{\rightarrow} 4 \mathrm{CO}_2(g) + 4 \mathrm{H}_2\mathrm{O}(g) \]

Equation b: Balance O Atoms

Now balance the oxygen atoms. There are 12 O atoms on the product side (8 from \(\mathrm{CO}_2\) and 4 from \(\mathrm{H}_2\mathrm{O}\)), so the balanced equation is: \[ \mathrm{C}_4\mathrm{H}_8(g) + 6 \mathrm{O}_2(g) \underset{\Delta}{\rightarrow} 4 \mathrm{CO}_2(g) + 4 \mathrm{H}_2\mathrm{O}(g) \]

Equation b: Identify Type of Reaction

This is a combustion reaction because a hydrocarbon reacts with oxygen to produce carbon dioxide and water.

Equation c: Initial Reaction

The given chemical equation is: \[\mathrm{Sb}(s) + \mathrm{Cl}_2(g) \rightarrow \mathrm{SbCl}_3(s)\]

Equation c: Balance the Equation

Count the Sb and Cl atoms. Both sides have 1 Sb and 3 Cl atoms, which means the equation is already balanced.

Equation c: Identify Type of Reaction

This is a synthesis (combination) reaction because two reactants combine to form a single product.

Equation d: Initial Reaction

The given chemical equation is: \[ \mathrm{NI}_3(s) \rightarrow \mathrm{N}_2(g) + \mathrm{I}_2(g) \]

Equation d: Balance the Equation

Balance the nitrogen and iodine atoms. The balanced equation is: \[ 2 \mathrm{NI}_3(s) \rightarrow 1 \mathrm{N}_2(g) + 3 \mathrm{I}_2(g) \]

Equation d: Identify Type of Reaction

This is a decomposition reaction because a single reactant breaks down into multiple products.

Equation e: Initial Reaction

The given chemical equation is: \[\mathrm{KBr}(aq) + \mathrm{Cl}_2(aq) \rightarrow \mathrm{KCl}(aq) + \mathrm{Br}_2(l)\]

Equation e: Balance the Equation

Count the K, Br, and Cl atoms. All are balanced as 1 K, 1 Br, and 2 Cl on both sides.

Equation e: Identify Type of Reaction

This is a single replacement reaction because one element (Cl) replaces another element (Br) in a compound.

Equation f: Initial Reaction

The given chemical equation is: \[\mathrm{Fe}(s) + \mathrm{H}_2\mathrm{SO}_4(aq) \rightarrow \mathrm{H}_2(g) + \mathrm{Fe}_2(\mathrm{SO}_4)_3(aq)\]

Equation f: Balance Fe, H, and S Atoms

Balance the atoms step-by-step. The balanced equation is: \[ 6 \mathrm{Fe}(s) + 6 \mathrm{H}_2\mathrm{SO}_4(aq) \rightarrow 3 \mathrm{H}_2(g) + 2 \mathrm{Fe}_2(\mathrm{SO}_4)_3(aq) \]

Equation f: Identify Type of Reaction

This is a redox reaction because there is a transfer of electrons between iron and sulfuric acid.

Equation g: Initial Reaction

The given chemical equation is: \[\mathrm{Al}_2(\mathrm{SO}_4)_3(aq) + \mathrm{NaOH}(aq) \rightarrow \mathrm{Al}(\mathrm{OH})_3(s) + \mathrm{Na}_2 \mathrm{SO}_4(aq)\]

Equation g: Balance Al, S, O and H Atoms

Balance the atoms step-by-step. The balanced equation is: \[ \mathrm{Al}_2(\mathrm{SO}_4)_3(aq) + 6 \mathrm{NaOH}(aq) \rightarrow 2 \mathrm{Al}(\mathrm{OH})_3(s) + 3 \mathrm{Na}_2\mathrm{SO}_4(aq) \]

Equation g: Identify Type of Reaction

This is a double displacement reaction because the anions and cations of the reactants swap places to form new compounds.

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Key Concepts

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

Combination Reaction

A combination reaction, also known as a synthesis reaction, involves two or more reactants combining to form a single product. These reactions are generally represented by the equation: \[ A + B \rightarrow AB \] where A and B are reactants, and AB is the product. In the exercise, the reactions \( \mathrm{NH}_3(g) + \mathrm{HCl}(g) \underset{\Delta}{\rightarrow} \mathrm{NH}_4\mathrm{Cl}(s) \) and \( \mathrm{Sb}(s) + \mathrm{Cl}_2(g) \rightarrow \mathrm{SbCl}_3(s) \) are examples. In both cases, two different reactants combine to form a single new compound. These reactions usually release energy and are exothermic.

Combustion Reaction

A combustion reaction is a type of chemical reaction in which a substance combines with oxygen, releasing a large amount of energy in the form of light and heat. Typically, hydrocarbons undergo combustion to produce carbon dioxide (\textrm{CO}_2}) and water (\textrm{H}_2O}). The general form of a combustion reaction is: \[ \mathrm{CxHy} + O_2 \rightarrow CO_2 + H_2O \] In the exercise, the equation \( \mathrm{C}_4\mathrm{H}_8(g) + \mathrm{O}_2(g) \underset{\Delta}{\rightarrow} 4 \mathrm{CO}_2(g) + 4 \mathrm{H}_2\mathrm{O}(g) \) serves as an example. Here, butene (C_4H_8) reacts with oxygen (O_2), producing carbon dioxide and water, demonstrating the typical combustion pattern.

Decomposition Reaction

A decomposition reaction occurs when a single compound breaks down into two or more simpler substances. This type of reaction is generally represented as: \[ AB \rightarrow A + B \] where AB is the reactant, and A and B are products. An example from the exercise is \( 2 \mathrm{NI}_3(s) \rightarrow 1 \mathrm{N}_2(g) + 3 \mathrm{I}_2(g) \). In this reaction, nitrogen triiodide (NI_3) decomposes into nitrogen (N_2) and iodine (I_2). Decomposition reactions usually require energy input in the form of heat, light, or electricity.

Single Replacement Reaction

A single replacement reaction, also known as a single displacement reaction, involves an element replacing another element in a compound. The general pattern is: \[ A + BC \rightarrow AC + B \] where A is a single element and BC is a compound. In the exercise, the equation \( \mathrm{KBr}(aq) + \mathrm{Cl}_2(aq) \rightarrow \mathrm{KCl}(aq) + \mathrm{Br}_2(l) \) illustrates this concept. Here, chlorine (Cl_2) replaces bromine (Br) in potassium bromide (KBr), resulting in the formation of potassium chloride (KCl) and bromine (Br_2). Single replacement reactions often occur in solutions.

Redox Reaction

Redox reactions, or oxidation-reduction reactions, involve the transfer of electrons between two substances. One substance gets oxidized (loses electrons), and the other gets reduced (gains electrons). The general representation is: \[ \text{Oxidation: } A \rightarrow A^{+} + e^{-} \] \[ \text{Reduction: } B + e^{-} \rightarrow B^{-} \] An example from the exercise is \( 6 \mathrm{Fe}(s) + 6 \mathrm{H}_2\mathrm{SO}_4(aq) \rightarrow 3 \mathrm{H}_2(g) + 2 \mathrm{Fe}_2(\mathrm{SO}_4)_3(aq) \). In this reaction, iron undergoes oxidation, and hydrogen ions get reduced, forming hydrogen gas. These reactions are essential in many biological and industrial processes.

Double Displacement Reaction

A double displacement reaction, also known as a metathesis reaction, involves the exchange of ions between two compounds to form two new compounds. The general equation is: \[ AB + CD \rightarrow AD + CB \] where AB and CD are the reactants, and AD and CB are the products. An example from the exercise is \( \mathrm{Al}_2(\mathrm{SO}_4)_3(aq) + 6 \mathrm{NaOH}(aq) \rightarrow 2 \mathrm{Al}(\mathrm{OH})_3(s) + 3 \mathrm{Na}_2 \mathrm{SO}_4(aq) \). In this case, aluminum sulfate (Al_2(SO_4)_3) exchanges ions with sodium hydroxide (NaOH), resulting in the formation of aluminum hydroxide (Al(OH)_3) and sodium sulfate (Na_2SO_4). These reactions often produce a precipitate when the two aqueous solutions mix.

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