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2 Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) PBCO3(s) PbO(s) + CO2(g) (b) C,H4(g) + O,(g) → CO2(g) + H,O(g) (c) Mg(s) + N2(g) – Mg;N2(s)

2 Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) PBCO3(s) PbO(s) + CO2(g) (b) C,H4(g) + O,(g) → CO2(g) + H,O(g) (c) Mg(s) + N2(g) – Mg;N2(s)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Balancing Chemical Equations and Classifying Reaction Types** **Exercise 3.22** Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) \( \text{PbCO}_3(s) \rightarrow \text{PbO}(s) + \text{CO}_2(g) \) (b) \( \text{C}_2\text{H}_4(g) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(g) \) (c) \( \text{Mg}(s) + \text{N}_2(g) \rightarrow \text{Mg}_3\text{N}_2(s) \) (d) \( \text{C}_7\text{H}_8\text{O}_2(l) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(g) \) (e) \( \text{Al}(s) + \text{Cl}_2(g) \rightarrow \text{AlCl}_3(s) \) **Instructions:** 1. **Balance Each Equation:** Adjust the coefficients to ensure that the number of atoms for each element is equal on both sides of the equation. 2. **Classify Each Reaction:** - **Combination Reaction:** Two or more substances combine to form one product. - **Decomposition Reaction:** A single compound breaks down into two or more simpler substances. - **Combustion Reaction:** Typically involves a hydrocarbon reacting with oxygen to produce carbon dioxide and water. **Note:** Each equation requires balancing for stoichiometric accuracy, indicating the law of conservation of mass is satisfied.
Transcribed Image Text:**Balancing Chemical Equations and Classifying Reaction Types** **Exercise 3.22** Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) \( \text{PbCO}_3(s) \rightarrow \text{PbO}(s) + \text{CO}_2(g) \) (b) \( \text{C}_2\text{H}_4(g) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(g) \) (c) \( \text{Mg}(s) + \text{N}_2(g) \rightarrow \text{Mg}_3\text{N}_2(s) \) (d) \( \text{C}_7\text{H}_8\text{O}_2(l) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(g) \) (e) \( \text{Al}(s) + \text{Cl}_2(g) \rightarrow \text{AlCl}_3(s) \) **Instructions:** 1. **Balance Each Equation:** Adjust the coefficients to ensure that the number of atoms for each element is equal on both sides of the equation. 2. **Classify Each Reaction:** - **Combination Reaction:** Two or more substances combine to form one product. - **Decomposition Reaction:** A single compound breaks down into two or more simpler substances. - **Combustion Reaction:** Typically involves a hydrocarbon reacting with oxygen to produce carbon dioxide and water. **Note:** Each equation requires balancing for stoichiometric accuracy, indicating the law of conservation of mass is satisfied.
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