If one gets oxidized by one Oxygen, the other one gets reduced by one Oxygen. You can get the reduced species in this way. Another way is by knowing the reaction mechanism. By the method I've followed here, you don't need to know the mechanism to solve the problem.
Hope that will help:-)
b) Balance the following reaction equations using the half-reaction method: 1. RCH2OH + H2Cro4 → RCO...
7 7) Balance the following redox equations using the half-reaction method. I. a Ag+ + b Zn → c Ag + d Zn2 a) What is coefficient a? b) What is coefficient b? a) What is coefficient c? b) What is coefficient d? c) How many electrons are transferred in the balanced equation? a Cu + b Au → Cu?! + d Au a) What is coefficient a? b) What is coefficient b? a) What is coefficient c? b) What...
(1) Balance the following oxidation–reduction reaction by the half-reaction method. (Use the lowest possible coefficients for the reaction.) CuCl2 (aq) + Zn (s) = Cu (s) + ZnCl2 (aq) (2) Balance the following oxidation–reduction reaction by the half-reaction method. (Use the lowest possible coefficients for the reaction.) H2 (g) + Ag+ (aq) = Ag (s) + H+ (aq)
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
Balance following redox reactions in acidic conditions using the half-reaction method a. Fe + Ag+ → Fe2+ + Ag b. I- + SO42- → H2S + I2 c. Cu + NO3- → Cu2+ + NO2 d. PbO₂ + CI- → Pb2+ + Cl₂
Balance the following ionic equations using the ion-electron method. Use H +1 and / or H2O, if necessary. Then identify the oxidation half-reaction and of reduction, the oxidizing agent and the reducing agent. 1. MnO4 - + H2C2O4 -2 → Mn + 2 + CO2 2. IO3 -1 + I-1 ⇌ I2 (ac)
1. Balance the following redox reaction using the method of half-reactions (also called the ion-electron method). Mn2+ (aq) + NaBiO3 (s) → Bi3+ (aq) + MnO4- (aq) + Na+ (aq) 2. Balance the following reaction is basic media. (remember you should have no H+ ions in your final reaction.) Pb(OH)42- (aq) + ClO- (aq) → PbO2 (s) + Cl- (aq)
2. Balance the following reaction that occurs in acid, using the half-reaction method. I-1(aq) + CrO4-1(aq) --> I2(s) + Cr+3(aq) When this reaction is balanced, there will be (?) H+(aq) and (?) H2O(l) in the final balanced equation. (Enter numbers without the plus sign.)
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
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO2(g) → NO,- (aq) (ii) (acid solution) H SeO(aq) → Se (s) (iii) (base solution) P (8) PH, (g) (iv) (base solution) Co(OH)(s) C002 () (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
Balance each of the following equations according to the half-reaction method: 1) CN- (aq) + ClO2( aq) —> CNO- (aq) + Cl- (aq) (in acid) 2) MnO4- (aq) +NO2- (aq) → MnO2( s) + NO3 - (aq) (in base) 3) In which species does nitrogen have the highest oxidation number? a) NaNO3 b) HNO2 c) NO2- d) NH3 e) N2