1. Balance the following using either method of balancing redox equations. Sn®+ Cr,0,2 -> Snº+ +...
1. Balance the following using either method of balancing redox equations. Sn2+ + Cr,0,2 > Sn"+ + Cr3+ (acid solution) DO osoba (rotulosban Ag,0 + CH,0 -> Ag + HCO," (basic solution) On 60405
Z homework points) Balancing Redox Equations Balance the following equation, using either the half-reaction method or the oxidation number method, and enter the coefficients in the boxes The coefficients must be the smallest possible integers All boxes must contain an entry. HNO3 + HI- 12 + H₂O + NO Submit Answer Tries 0/5 e Post Discussion Type here to search e D Caps Shift х M Ctrl
Balancing redox equations: Complete and balance the following redox equation occurring in aqueous solution. C2O42− + BrO3− → CO2 (g) + Br−
Using the rules for balancing redox equations either from your textbook or from lecture, balance KIO3(aq) + KI(aq) + H2SO4(aq) -----> I2(aq) + K2SO4 I2(aq) + Na2S2O3(aq) ---------> NaI(aq) + Na2S4O6(aq) . Note that these are molecular equations that use neutral chemical formulas and that the reactions occur in an acidic medium as indicated by the presence of sulfuric acid. It may be easier to “remove” the spectator ions and write the net ionic equation before you balance (Hint: Na+ and...
Reduce Simple Redux Equation This method of balancing reaction is called the half reaction method. Balance the following redox reaction Na (s) + Ap, (aq) → Na, (aq) + Al (s) Balance the following redox reaction Sn2. (aq) + Fe3. (aq) → Sn°. (aq) + Fe2+ (aq) Balance the following redox reaction Cr3' (aq) + Cl. (aq) → Cl2 (g) + Cr (s)
Balance the following Redox Equations in Basic Mediums. Redox Reactions in Basic Solution 1. Al(s) + MnO4¯ (aq) ¾® MnO2(s) + Al(OH)4¯ (aq) 2. NO2¯ (aq) + Al(s) ¾® NH3(aq) + AlO2¯ (aq) 3. Cr(s) + CrO42-(aq) ¾® Cr(OH)3(s) Note: Cr(OH)3 is found in BOTH half reactions! 4. Cl2(aq) + Br2(l) ¾® OBr¯ (aq) + Cl¯ (aq) 5. S8(aq) + MnO4¯ (aq) ¾® SO42-(aq) + MnO2(s)
Assignment 6.3-Balancing Redox Reactions 1 Balance the following reactions using the oxidation number method (fill in table as wel) a. NaClO+ H2S ? NaCl+ H2SO4 Element Initial Oxidation # Final Oxidation # Reduced or Oxidized? Element initial Oxidation # Final Oxidation # Reduced or Oxidized? K2Cr:07 + SnCl2 + HCl? CrCb + SnCl4 + KCl + H2O Element Initial Oxidation # Final Oodation # Reduced or Oxidized? 2. Balance the following half-reactions. Be sure to balance for atoms first, then...
3. Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): Cr0(aq) + U" (aq) → Cr" (aq) +UO; (aq) (b) (acid solution): Cr(s) + O2(g) → Cr* (aq) (C) (basic solution): P. (s) + OH' (aq) → PH; (g) + H2PO2 (aq)
Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): VŽ+ + V(OH). - VO2 (b) (acid solution): C 02 + MnO - CO2(g) + Mn (c) (basic solution): Cr(OH), (s) + H2O2 → CrO
Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): MnO2 (s) + Cl → Mn2+ + Cl2 (g) (b) (acid solution): NaBiO; (s) + Ce3+ BiO+ + Ce4+ + Na+ (c) (basic solution): Fe(OH)2 (s) + CrO42- → Fe,0, (s) + Cr(OH)4