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Chapter 22: Problem 65

Complete and balance the following equations: (a) \(\mathrm{ZnCO}_{3}(s) \stackrel{\Delta}{\longrightarrow}\) (b) \(\mathrm{BaC}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (c) \(\mathrm{C}_{2} \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow\) (d) \(\mathrm{CS}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow\) (e) \(\mathrm{Ca}(\mathrm{CN})_{2}(s)+\operatorname{HBr}(a q) \longrightarrow\)

Short Answer

Expert verified
(a) \( ZnCO_3(s) \stackrel{\Delta}{\longrightarrow} ZnO(s) + CO_2(g) \) (b) \( BaC_2(s) + 2 H_2O(l) \longrightarrow Ba(OH)_2(s) + C_2H_2(g) \) (c) \( 2 C_2H_2(g) + 5 O_2(g) \longrightarrow 4 CO_2(g) + 4 H_2O(g) \) (d) \( CS_2(g) + 3 O_2(g) \longrightarrow CO_2(g) + 2 SO_2(g) \) (e) \( Ca(CN)_2(s) + 2 HBr(aq) \longrightarrow CaBr_2(aq) + 2 HCN(aq) \)

Step by step solution

01

Balance equation (a)

(a) ZnCO3(s) 鈫� ZnO(s) + CO2(g) Since there is 1 Zn, 1 C, and 3 O atoms on both sides of the equation, it is already balanced.
02

Balance equation (b)

(b) BaC2(s) + H2O(l) 鈫� Ba(OH)2(s) + C2H2(g) First, balance the Ba atoms: 1 Ba on both sides, no change needed. Next, balance the C atoms: 2 C on the left, 2 C on the right, no change needed. Finally, balance the H and O atoms by placing a "2" in front of H2O and Ba(OH)2: BaC2(s) + 2 H2O(l) 鈫� Ba(OH)2(s) + C2H2(g)
03

Balance equation (c)

(c) C2H2(g) + O2(g) 鈫� CO2(g) + H2O(g) First, balance the C atoms by placing a "2" in front of CO2: C2H2(g) + O2(g) 鈫� 2 CO2(g) + H2O(g) Next, balance the H atoms by placing a "2" in front of H2O: C2H2(g) + O2(g) 鈫� 2 CO2(g) + 2 H2O(g) Finally, balance the O atoms by placing a "5/2" in front of O2 and multiplying all coefficients by 2: 2 C2H2(g) + 5 O2(g) 鈫� 4 CO2(g) + 4 H2O(g)
04

Balance equation (d)

(d) CS2(g) + O2(g) 鈫� CO2(g) + SO2(g) First, balance the C atoms: 1 C on both sides, no change needed. Next, balance the S atoms by placing a "2" in front of SO2: CS2(g) + O2(g) 鈫� CO2(g) + 2 SO2(g) Finally, balance the O atoms by placing a "3" in front of O2: CS2(g) + 3 O2(g) 鈫� CO2(g) + 2 SO2(g)
05

Balance equation (e)

(e) Ca(CN)2(s) + HBr(aq) 鈫� CaBr2(aq) + HCN(aq) First, balance the Ca atoms: 1 Ca on both sides, no change needed. Next, balance the Br atoms by placing a "2" in front of HBr and CaBr2: Ca(CN)2(s) + 2 HBr(aq) 鈫� CaBr2(aq) + HCN(aq) Finally, balance the C and N atoms by placing a "2" in front of HCN: Ca(CN)2(s) + 2 HBr(aq) 鈫� CaBr2(aq) + 2 HCN(aq)

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Key Concepts

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

Balancing Chemical Reactions
To understand balancing chemical reactions, it is crucial to grasp the concept of the law of conservation of mass. This law states that matter is neither created nor destroyed in a chemical reaction. Balancing chemical equations ensures that this law is followed. Each type of atom present in the reactants must be equal to those in the products.
  • Start by identifying all reactants and products involved.
  • Count the number of each type of atom on both sides of the equation.
  • Add coefficients to the compounds in the equation to equalize the number of each type of atom on both sides.
  • Adjust and repeat the process as needed until balanced.
By following these steps, you will ensure that your chemical equations reflect the real-world changes occurring during a reaction.
Chemical Decomposition
Chemical decomposition is a type of reaction where a single compound breaks down into two or more simpler substances. This process is usually initiated by heating, voltage, or a catalyst. In the provided exercise, equation (a) represents a decomposition reaction:
ZnCOe needs to heat back up 3(s) \( \longrightarrow \) ZnO(s) + COdisemination2(g).
Key points to remember about decomposition reactions include:
  • Typically, they require energy in the form of heat, light, or electricity.
  • Often involve a single reactant.
  • Produces multiple simpler products like elements or simpler compounds.
Decomposition reactions are prevalent in various fields, such as the decomposition of carbonates to form oxides and carbon dioxide.
Combustion Reactions
Combustion reactions are characterized by the process of burning, where a substance reacts rapidly with oxygen to release energy. These reactions produce heat and light, making them exothermic. In the steps provided, equation (c) illustrates a combustion reaction:
Cdisemination2Hdisemination2(g) + Odisemination2(g) \( \longrightarrow \) COdisemination2(g) + Hdisemination2O(g).
Important features of combustion reactions include:
  • Reactants typically include a hydrocarbon and oxygen.
  • Products are usually carbon dioxide and water.
  • They are a significant source of energy in everyday contexts, such as power plants and engines.
Understanding combustion reactions can help in exploring energy production and initiating further studies on sustainable energy sources.
Stoichiometry
Stoichiometry is the area of chemistry that involves quantitative relationships between reactants and products in a chemical reaction. It is essential for predicting how much of a product will form and reactant will be needed.
To approach stoichiometry, follow these steps:
  • Ensure the chemical equation is balanced, as seen in all equations from the exercise.
  • Use the balanced equation to derive mole ratios between reactants and products.
  • Apply these mole ratios to convert between masses, moles, or even particles of the reactants and products.
Overall, stoichiometry enables chemists to perform practical and calculated predictions, critical in both laboratory and industrial applications, ensuring efficient use of resources.

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Most popular questions from this chapter

Identify the true statements concerning the atoms and ions of the group 16 elements. [Sections 22.5 and 22.6\(]\) (a) The ionic radii are larger than the atomic radii because the ions have more electrons than their corresponding atoms. (b) Atomic radii increase going down the group because of increasing nuclear charge. (c) The ionic radii increase going down the group because of the increase in the principal quantum number of outermost electrons. (d) Of these ions, \(\mathrm{Se}^{2-}\) is the strongest base in water because it is largest.

Write the chemical formula for each of the following, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) xenon trioxide difluoride, \((\mathbf{b})\) chlorine dioxide, \((\mathbf{c})\) molybdenum hexafluoride, \((\mathbf{d})\) iodic acid, (e) sodium hypobromite, \((\mathbf{f})\) magnesium iodite.

Which of the following statements are true? (a) Si can form an ion with six fluorine atoms, \(\mathrm{SiF}_{6}^{2-}\), whereas carbon cannot. (b) Si can form three stable compounds containing two \(\mathrm{Si}\) atoms each, \(\mathrm{Si}_{2} \mathrm{H}_{2}, \mathrm{Si}_{2} \mathrm{H}_{4},\) and \(\mathrm{Si}_{2} \mathrm{H}_{6}\) (c) In \(\mathrm{HNO}_{3}\) and \(\mathrm{H}_{3} \mathrm{PO}_{4}\) the central atoms, \(\mathrm{N}\) and \(\mathrm{P}\), have different oxidation states. (d) \(\mathrm{S}\) is more electronegative than Se.

Ultrapure germanium, like silicon, is used in semiconductors. Germanium of "ordinary" purity is prepared by the high-temperature reduction of \(\mathrm{GeO}_{2}\) with carbon. The Ge is converted to \(\mathrm{GeCl}_{4}\) by treatment with \(\mathrm{Cl}_{2}\) and then purified by distillation; \(\mathrm{GeCl}_{4}\) is then hydrolyzed in water to \(\mathrm{GeO}_{2}\) and reduced to the elemental form with \(\mathrm{H}_{2}\). The element is then zone refined. Write a balanced chemical equation for each of the chemical transformations in the course of forming ultrapure Ge from \(\mathrm{GeO}_{2}\).

Write complete balanced half-reactions for (a) oxidation of nitrous acid to nitrate ion in acidic solution, (b) oxidation of \(\mathrm{N}_{2}\) to \(\mathrm{N}_{2} \mathrm{O}\) in acidic solution.
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