Ch.3 - Chemical Reactions and Reaction Stoichiometry

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 11c

Chapter 3, Problem 11c

Balance the following equations: c. CH4(𝑔)+Cl2(𝑔)⟶CCl4(𝑙)+HCl(𝑔)

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Identify the number of each type of atom on both sides of the equation. Initially, you have: Reactants: 1 C, 4 H, 2 Cl; Products: 1 C, 1 Cl, 1 H.

Notice that the carbon atoms are already balanced with 1 C on each side.

Balance the chlorine atoms. You have 2 Cl in Cl2 on the reactant side and 4 Cl in CCl4 on the product side. To balance, you need 4 Cl on the reactant side, so multiply Cl2 by 2.

Now, balance the hydrogen atoms. You have 4 H in CH4 on the reactant side and 1 H in HCl on the product side. To balance, multiply HCl by 4.

Check the balance: Reactants: 1 C, 4 H, 4 Cl; Products: 1 C, 4 Cl, 4 H. The equation is now balanced.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, coefficients are adjusted in front of the chemical formulas to achieve equal atom counts.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows chemists to predict the amounts of substances consumed and produced in a reaction based on balanced equations. Understanding stoichiometry is essential for calculating yields, determining limiting reactants, and performing conversions between moles and grams.

States of Matter

The states of matter refer to the distinct forms that different phases of matter take on, primarily solid, liquid, and gas. In chemical equations, the physical state of each substance is indicated by symbols: (s) for solid, (l) for liquid, and (g) for gas. Recognizing these states is important for understanding the behavior of substances during reactions and for accurately representing the reaction conditions.

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Related Practice

Textbook Question

A key step in balancing chemical equations is correctly identifying the formulas of the reactants and products. For example, consider the reaction between calcium oxide, CaO(s), and H2O1l2 to form aqueous calcium hydroxide. (b) Is it possible to balance the equation if you incorrectly identify the product as CaOH1aq2, and if so, what is the equation?

Textbook Question

Write 'true' or 'false' for each statement. (a) We balance chemical equations as we do because energy must be conserved.

Textbook Question

Balance the following equations: d. AlCl3(𝑠)+Ca3N2(𝑠)⟶AlN(𝑠)+CaCl2(𝑠)

Textbook Question

Balance the following equations: c. NH4NO3(𝑠)⟶N2(𝑔)+O2(𝑔)+H2O(𝑔)

Textbook Question

Write 'true' or 'false' for each statement. (b) If the reaction 2 O₃(g) → 3 O₂(g) goes to completion and all O₃ is converted to O₂, then the mass of O₃ at the beginning of the reaction must be the same as the mass of O₂ at the end of the reaction.

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Textbook Question

Balance the following equations: b. TiCl4(𝑙)+H2O(𝑙)⟶TiO2(𝑠)+HCl(𝑎𝑞)