/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 81 Write the balanced chemical equa... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 3: Problem 81

Write the balanced chemical equatiuns fur (a) the complete combustion of acetic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\), the main active ingredient in vinegar; (b) the decomposition of solid calcium hydroxide into solid calcium(II) oxide (lime) and water vapor; (c) the combination reaction between nickel metal and chlorine gas.

Short Answer

Expert verified
The balanced chemical equations for each reaction are: a) Complete combustion of acetic acid: \(2 \mathrm{CH}_{3}\mathrm{COOH}+O_{2} \rightarrow 2 \mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O}\) b) Decomposition of solid calcium hydroxide: \(\mathrm{Ca}(\mathrm{OH})_{2} \rightarrow \mathrm{CaO}+\mathrm{H}_{2} \mathrm{O}\) c) Combination reaction between nickel metal and chlorine gas: \(\mathrm{Ni}+2 \mathrm{Cl}_{2} \rightarrow \mathrm{NiCl}_{2}\)

Step by step solution

01

Determine the products for each reaction.

Before we balance the equations, we need to identify the products of each reaction: a) Complete combustion reactions involve the reaction of a compound with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). b) Decomposition reactions involve a single compound breaking down into two or more simpler substances. c) Combination reactions involve two or more substances joining to form a single compound.
02

Write the unbalanced chemical equations.

Next, we write the unbalanced equations for each reaction, based on our knowledge of the reactants and products: a) CH3COOH + O2 鈫� CO2 + H2O b) Ca(OH)2 鈫� CaO + H2O c) Ni + Cl2 鈫� NiCl2
03

Balance the chemical equations.

Now, we balance each equation by adjusting the coefficients (the numbers in front of each compound) to ensure that the number of each element is equal on both sides: a) Combustion of acetic acid: - We need 2 carbon atoms and 4 hydrogen atoms on both sides. - The balanced equation becomes: \(2 \mathrm{CH}_{3}\mathrm{COOH}+O_{2} \rightarrow 2 \mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O}\) b) Decomposition of calcium hydroxide: - The equation is already balanced: \(\mathrm{Ca}(\mathrm{OH})_{2} \rightarrow \mathrm{CaO}+\mathrm{H}_{2} \mathrm{O}\) c) Combination of nickel and chlorine: - We need 2 chlorine atoms on both sides. - The balanced equation becomes: \(\mathrm{Ni}+2 \mathrm{Cl}_{2} \rightarrow \mathrm{NiCl}_{2}\)
04

Summary of balanced chemical equations

The balanced chemical equations for each reaction are as follows: a) Complete combustion of acetic acid: \(2 \mathrm{CH}_{3}\mathrm{COOH}+O_{2} \rightarrow 2 \mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O}\) b) Decomposition of solid calcium hydroxide: \(\mathrm{Ca}(\mathrm{OH})_{2} \rightarrow \mathrm{CaO}+\mathrm{H}_{2} \mathrm{O}\) c) Combination reaction between nickel metal and chlorine gas: \(\mathrm{Ni}+2 \mathrm{Cl}_{2} \rightarrow \mathrm{NiCl}_{2}\)

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

Complete Combustion
Complete combustion refers to a type of chemical reaction where a compound, typically a hydrocarbon, reacts with an excess of oxygen to produce carbon dioxide, water, and energy. This reaction is commonly used in engines and power plants to generate heat and power. For instance, the combustion of acetic acid (CH_{3}COOH) in excess oxygen produces carbon dioxide and water, releasing heat in the process.
It is crucial that there is enough oxygen available for complete combustion to occur; otherwise, incomplete combustion may result, leading to the production of carbon monoxide and possibly soot. This could have harmful environmental and health impacts.
Decomposition Reaction
A decomposition reaction involves the breakdown of a compound into two or more simpler substances. Generally, this type of reaction requires an input of energy, such as heat, light, or electricity. For example, calcium hydroxide (Ca(OH)_2) decomposes into calcium oxide (lime) and water vapor when heated. This process is integral in various industries, including construction where lime is a key component in cement and mortar. Decomposition reactions are also important for recycling materials and understanding degradation processes in the environment.
Combination Reaction
Combination reactions, also known as synthesis reactions, occur when two or more reactants combine to form a single product. This fundamental type of chemical reaction is seen in various processes, from the formation of compounds in stars to the synthesis of molecules in living organisms. A classic example is the reaction between nickel metal and chlorine gas to form nickel(II) chloride. In combination reactions, the reactants may be elements or compounds and can vary from simple to very complex structures.
Balanced Chemical Equation
Writing a balanced chemical equation is an essential skill in chemistry as it ensures the law of conservation of mass is respected. To balance a chemical equation, the number of atoms for each element must be the same on both sides of the reaction. This is achieved by placing coefficients in front of the chemical formulas. A perfectly balanced equation allows one to accurately calculate the quantities required for a reaction and the expected yield. Additionally, it provides deeper insight into the stoichiometric relationships between reactants and products, which is pivotal in reaction stoichiometry.
Reactants and Products
In any given chemical reaction, substances that undergo the transformation are known as reactants, while substances that are generated by the reaction are called products. During a chemical reaction, the reactants are consumed to form the products, but the total mass and the number of atoms remain conserved. Understanding the reactants and products in a reaction simplifies the learning of chemical processes and assists in predicting the outcomes of reactions, which is crucial for applications across chemistry, biology, environmental science, and engineering.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Balance the following equations, and indicate whether they are combination, decomposition, or combustion reactions: (a) \(\mathrm{Al}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{AlCl}_{3}(s)\) (b) \(\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) (c) \(\mathrm{Li}(s)+\mathrm{N}_{2}(g) \longrightarrow \mathrm{Li}_{3} \mathrm{~N}(s)\) (d) \(\mathrm{PbCO}_{3}(s) \longrightarrow \mathrm{PbO}(s)+\mathrm{CO}_{2}(g)\) (e) \(\mathrm{C}_{7} \mathrm{H}_{8} \mathrm{O}_{2}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\)

(a) What scientific principle or law is used in the process of balancing chemical equations? (b) In balancing equations, why should you not change subscripts in chemical formulas? (c) How would one write out liquid water, water vapor, aqueous sodium chloride, and solid sodium chloride in chemical equations?

Withoutdoing any detailed calculations (but using a periodic table to give atomic weights), rank the following samples in order of increasing number of atoms: \(3.0 \times 10^{23}\) molecules of \(\mathrm{H}_{2} \mathrm{O}_{2}, 2.0 \mathrm{~mol} \mathrm{CH}_{4}, 32 \mathrm{~g} \mathrm{O}_{2}\)

(a) When the metallic element sodium combines with the nonmetallic element bromine, \(\mathrm{Br}_{2}(l)\), how can you determine the chemical formula of the product? How do you know whether the product is a solid, liquid, or gas at room temperature? Write the balanced chemical equation for the reaction. (b) When a hydrocarbon burns in air, what reactant besides the hydrocarbon is involved in the reaction? What products are formed? Write a balanced chemical equation for the combustion of benzene, \(\mathrm{C}_{6} \mathrm{H}_{6}(I)\), in air.

Epsom salts, a strong laxative used in veterinary medicine, is a hydrate, which means that a certain number of water molecules are included in the solid structure. The formula for Epsom salts can be written as \(\mathrm{MgSO}_{4} \cdot x \mathrm{H}_{2} \mathrm{O}\), where \(x\) indicates the number of moles of \(\mathrm{H}_{2} \mathrm{O}\) per mole of \(\mathrm{MgSO}_{4}\). When \(5.061 \mathrm{~g}\) of this hydrate is heated to \(250{ }^{\circ} \mathrm{C}\), all the water of hydration is lost, leaving \(2.472 \mathrm{~g}\) of \(\mathrm{MgSO}_{4}\). What is the value of \(x\) ?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Kinetics

Read Explanation

The Earths Atmosphere

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Inorganic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.