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Complete and balance the following half-reactions. Cr* (aq) Cr**(aq) а. b. Hg(1) + Br HgBr MnO2(s) MnO4 (aq) (in basic solution) c. d. CF (aq) clo: (aq) (in acidic solution)

Complete and balance the following half-reactions. Cr* (aq) Cr**(aq) а. b. Hg(1) + Br HgBr MnO2(s) MnO4 (aq) (in basic solution) c. d. CF (aq) clo: (aq) (in acidic solution)

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
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### Balancing Half-Reactions This section covers how to balance different half-reactions, which is crucial in redox chemistry. Below are some half-reactions that need to be balanced under specified conditions. #### Problems 1. **Reaction a:** \( \text{Cr}^{2+} \text{(aq)} \rightarrow \text{Cr}^{3+} \text{(aq)} \) This reaction involves the chromium ion changing its oxidation state from +2 to +3 in an aqueous solution. 2. **Reaction b:** \( \text{Hg(l)} + \text{Br}^- \rightarrow \text{HgBr}_2^{2-} \) Here, liquid mercury reacts with bromide ions to form mercury dibromide anion. 3. **Reaction c:** \( \text{MnO}_2 \text{(s)} \rightarrow \text{MnO}_4^-\text{(aq)} \) *(in basic solution)* Manganese dioxide in solid form is being converted into a permanganate ion in a basic solution. 4. **Reaction d:** \( \text{Cl}^- \text{(aq)} \rightarrow \text{ClO}_3^- \text{(aq)} \) *(in acidic solution)* Chloride ion in an aqueous solution is being oxidized to chlorate ion in the presence of an acidic medium. #### Detailed Steps to Balance Half-Reactions: - **Identify Oxidation Numbers:** Determine the oxidation states of each element in the reactants and products. - **Balance Atoms:** Other than hydrogen and oxygen, make sure all other atoms are balanced. - **Balance Oxygen Atoms:** Use water (H2O) to balance the oxygen atoms. - **Balance Hydrogen Atoms:** Use hydrogen ions (H+) to balance hydrogen atoms when in acidic solutions. For basic solutions, use water (H2O) and hydroxide ions (OH-) to balance hydrogen and oxygen atoms. - **Balance Charge:** Finally, add electrons (e-) to one side of the equation to balance the overall charge on both sides. Understanding these steps and practicing them with the reactions given above will enhance your skills in balancing chemical equations, especially for redox reactions.
Transcribed Image Text:### Balancing Half-Reactions This section covers how to balance different half-reactions, which is crucial in redox chemistry. Below are some half-reactions that need to be balanced under specified conditions. #### Problems 1. **Reaction a:** \( \text{Cr}^{2+} \text{(aq)} \rightarrow \text{Cr}^{3+} \text{(aq)} \) This reaction involves the chromium ion changing its oxidation state from +2 to +3 in an aqueous solution. 2. **Reaction b:** \( \text{Hg(l)} + \text{Br}^- \rightarrow \text{HgBr}_2^{2-} \) Here, liquid mercury reacts with bromide ions to form mercury dibromide anion. 3. **Reaction c:** \( \text{MnO}_2 \text{(s)} \rightarrow \text{MnO}_4^-\text{(aq)} \) *(in basic solution)* Manganese dioxide in solid form is being converted into a permanganate ion in a basic solution. 4. **Reaction d:** \( \text{Cl}^- \text{(aq)} \rightarrow \text{ClO}_3^- \text{(aq)} \) *(in acidic solution)* Chloride ion in an aqueous solution is being oxidized to chlorate ion in the presence of an acidic medium. #### Detailed Steps to Balance Half-Reactions: - **Identify Oxidation Numbers:** Determine the oxidation states of each element in the reactants and products. - **Balance Atoms:** Other than hydrogen and oxygen, make sure all other atoms are balanced. - **Balance Oxygen Atoms:** Use water (H2O) to balance the oxygen atoms. - **Balance Hydrogen Atoms:** Use hydrogen ions (H+) to balance hydrogen atoms when in acidic solutions. For basic solutions, use water (H2O) and hydroxide ions (OH-) to balance hydrogen and oxygen atoms. - **Balance Charge:** Finally, add electrons (e-) to one side of the equation to balance the overall charge on both sides. Understanding these steps and practicing them with the reactions given above will enhance your skills in balancing chemical equations, especially for redox reactions.
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