Redox Reaction: Cr(OH)3 + Br2 → CrO42- + Br- Explanation: This redox reaction involves the oxidation of Cr(OH)3 (chromium hydroxide) by bromine (Br2) and the reduction of bromine to form bromide (Br-). The oxidation of chromium hydroxide results in the formation of chromate (CrO42-). Balanced Half Equations: Cr(OH)3 → CrO42- + 2e- (oxidation) Br2 + 2e- → 2Br- (reduction) Oxidizing Agent: Bromine (Br2) Reducing Agent: Chromium Hydroxide (Cr(OH)3) Hazards and Application Methods: Chromium Hydroxide is a corrosive alkaline substance and can cause skin and eye irritations. Bromine is a toxic and corrosive substance and inhaling its fumes can cause serious respiratory problems. Therefore, it is important to wear protective equipment (goggles, gloves, and clothing) when handling both of these chemicals. It is also important to work in a well-ventilated area. When mixing the two chemicals, it is important to add the Bromine to the Chromium Hydroxide slowly and to stir the mixture continuously to ensure that the reaction is complete. Similar Examples: Example 1: Redox Reaction: MnO4- + Fe2+ → Mn2+ + Fe3+ Explanation: This redox reaction involves the oxidation of Iron (Fe2+) by Manganate (MnO4-) and the reduction of Manganate to form Manganese (Mn2+). The oxidation of Iron results in the formation of Ferrate (Fe3+). Balanced Half Equations: MnO4- → Mn2+ + 4e- (oxidation) Fe2+ + 2e- → Fe3+ (reduction) Oxidizing Agent: Manganate (MnO4-) Reducing Agent: Iron (Fe2+) Hazards and Application Methods: Manganate is a corrosive alkaline substance and can cause skin and eye irritations. Iron is a toxic and corrosive substance and inhaling its fumes can cause serious respiratory problems. Therefore, it is important to wear protective equipment (goggles, gloves, and clothing) when handling both of these chemicals. It is also important to work in a well-ventilated area. When mixing the two chemicals, it is important to add the Manganate to the Iron slowly and to stir the mixture continuously to ensure that the reaction is complete. Example 2: Redox Reaction: K2S2O8 + I2 → KI + K2SO4 Explanation: This redox reaction involves the oxidation of Iodine (I2) by Potassium Peroxydisulfate (K2S2O8) and the reduction of Potassium Peroxydisulfate to form Potassium Iodide (KI) and Potassium Sulfate (K2SO4). The oxidation of Iodine results in the formation of Iodide (I-). Balanced Half Equations: K2S2O8 → K2SO4 + 2I- + 4e- (oxidation) I2 + 2e- → 2I- (reduction) Oxidizing Agent: Potassium Peroxydisulfate (K2S2O8) Reducing Agent: Iodine (I2) Hazards and Application Methods: Potassium Peroxydisulfate is a corrosive alkaline substance and can cause skin and eye irritations. Iodine is a toxic and corrosive substance and inhaling its fumes can cause serious respiratory problems. Therefore, it is important to wear protective equipment (goggles, gloves, and clothing) when handling both of these chemicals. It is also important to work in a well-ventilated area. When mixing the two chemicals, it is important to add the Potassium Peroxydisulfate to the Iodine slowly and to stir the mixture continuously to ensure that the reaction is complete.