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1. 2. 3. 4. 5. 6. Rules for Balancing Redox Equations Write the skeleton equation for the reaction. Assign oxidation numbers to all elements and determine what is being oxidized and what is being reduced. Ignore everything else for now. Write the electronic equations for the oxidation and reduction processes. Adjust the coefficients in both equations so that the number of electrons lost equals the number of electrons gained. Place these coefficients back into the skeleton equation. Now balance the entire equation for conservation of atoms. Cl2 à 1. Fe + 2. KOH + Cl2 à 3. H2 4. Cl2 5. KI + 6. H2S 7. HNO3 8. H2S + O2 9. H2S 10 HNO3 11. KMnO4 12. CuS + I2 13. As2S5 + HNO3 14. H2SO4 + HI à 15. HNO3 + S à 16. CrCl3 + MnO2 17. KMnO4 18. HNO3 + S à 19. HNO3 + H2S 20. HNO3 + P à + Cl2 FeCl3 KClO3 à HCl + H2O à Br2 + HCl + HClO à KBr + I2 à Cl2 S à HCl H2O + S + NO S + H2O à Br2 + à + H2S + + KCl + H2O S + CuS à + HBr NO2 + HCl à Cl2 + HCl à à + Cu(NO3)2 + H2O + SO2 + KCl + H2O + MnCl2 S + HI + NO2 CuCl2 + H2O + H3AsO4 + H2SO4 H2S + H2O + I2 NO2 + H2SO4 + H2O à + HCl + H2S à + H2O MnCl2 + H2CrO4 KCl + MnCl2 NO + H2SO4 à H2SO4 H3PO4 + NO2 + NO2 + H2O + H2O + S + H2O