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 22a

Chapter 3, Problem 22a

Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: a. PbCO3(s) → PbO(s) + CO2(g)

Verified step by step guidance

Step 1: Identify the type of reaction. In this case, the reaction is a decomposition reaction. This is because a single compound (PbCO3) is breaking down into simpler substances (PbO and CO2).

Step 2: Balance the equation. Start by balancing the elements that appear in only one compound on each side. In this case, we can start with Pb. There is one Pb atom on both sides, so it is already balanced.

Step 3: Next, balance the carbon atoms. There is one carbon atom on both sides, so it is also already balanced.

Step 4: Finally, balance the oxygen atoms. There are 3 oxygen atoms on the left side (from PbCO3) and 3 on the right side (1 from PbO and 2 from CO2), so they are also balanced.

Step 5: Check your work. The balanced equation is PbCO3(s) → PbO(s) + CO2(g), and all atoms are balanced on both sides of the equation. Therefore, the equation is correctly 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. Balancing is crucial for accurately representing the reaction and predicting the amounts of reactants and products.

Types of Chemical Reactions

Chemical reactions can be classified into several types, including combination, decomposition, and combustion reactions. A combination reaction occurs when two or more substances combine to form a single product. A decomposition reaction involves a single compound breaking down into two or more simpler products, while combustion reactions typically involve a substance reacting with oxygen to produce heat and light, often resulting in carbon dioxide and water.

Decomposition Reactions

Decomposition reactions are a specific type of chemical reaction where a single compound breaks down into two or more simpler substances. This process often requires energy input, such as heat, light, or electricity. In the given equation, PbCO3 decomposes into PbO and CO2, illustrating this concept as it transitions from one compound to multiple products.

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