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4. Balance the following reactions, using coefficients, and label the type of reaction (combination, decomposition, single-replacement, double-replacement, or combustion). a) Cr + 02 > Cr2O3 b) CSH12 + 02 → CO2 + H2O c) N2O5 > NO2 + O2 d) AGNO3 + MgCl2 → AgCl Mg(NO3)2 e) Sn + HCI -> SnCl2 + H2

4. Balance the following reactions, using coefficients, and label the type of reaction (combination, decomposition, single-replacement, double-replacement, or combustion). a) Cr + 02 > Cr2O3 b) CSH12 + 02 → CO2 + H2O c) N2O5 > NO2 + O2 d) AGNO3 + MgCl2 → AgCl Mg(NO3)2 e) Sn + HCI -> SnCl2 + H2

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 Reactions** The following reactions need to be balanced using coefficients. Once balanced, classify each reaction type as combination, decomposition, single-replacement, double-replacement, or combustion. a) \( \text{Cr} + \text{O}_2 \rightarrow \text{Cr}_2\text{O}_3 \) b) \( \text{C}_5\text{H}_{12} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \) c) \( \text{N}_2\text{O}_5 \rightarrow \text{NO}_2 + \text{O}_2 \) d) \( \text{AgNO}_3 + \text{MgCl}_2 \rightarrow \text{AgCl} + \text{Mg(NO}_3\text{)}_2 \) e) \( \text{Sn} + \text{HCl} \rightarrow \text{SnCl}_2 + \text{H}_2 \) **Instructions:** 1. Add the appropriate coefficients to each reactant and product to balance the equations. 2. Identify the type of reaction for each equation: - **Combination:** Two or more substances combine to form a single product. - **Decomposition:** A single compound breaks down into two or more simpler substances. - **Single-replacement:** An element replaces a similar element in a compound. - **Double-replacement:** The ions of two compounds exchange places in an aqueous solution to form two new compounds. - **Combustion:** A substance combines with oxygen, releasing a large amount of energy in the form of light and heat. **Note:** There are no graphs or diagrams associated with these reactions.
Transcribed Image Text:**Balancing Chemical Reactions** The following reactions need to be balanced using coefficients. Once balanced, classify each reaction type as combination, decomposition, single-replacement, double-replacement, or combustion. a) \( \text{Cr} + \text{O}_2 \rightarrow \text{Cr}_2\text{O}_3 \) b) \( \text{C}_5\text{H}_{12} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \) c) \( \text{N}_2\text{O}_5 \rightarrow \text{NO}_2 + \text{O}_2 \) d) \( \text{AgNO}_3 + \text{MgCl}_2 \rightarrow \text{AgCl} + \text{Mg(NO}_3\text{)}_2 \) e) \( \text{Sn} + \text{HCl} \rightarrow \text{SnCl}_2 + \text{H}_2 \) **Instructions:** 1. Add the appropriate coefficients to each reactant and product to balance the equations. 2. Identify the type of reaction for each equation: - **Combination:** Two or more substances combine to form a single product. - **Decomposition:** A single compound breaks down into two or more simpler substances. - **Single-replacement:** An element replaces a similar element in a compound. - **Double-replacement:** The ions of two compounds exchange places in an aqueous solution to form two new compounds. - **Combustion:** A substance combines with oxygen, releasing a large amount of energy in the form of light and heat. **Note:** There are no graphs or diagrams associated with these reactions.
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