or the oxidation-reduction reactions in the disinfection tank containing ammonium: NH4+ + 4Cl2 (g) + 3H2O == NO3- + 8Cl- + 10H+, the oxidation number of N in NH4+ is
–3 |
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+3 |
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–4 |
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+4 |
or the oxidation-reduction reactions in the disinfection tank containing ammonium: NH4+ + 4Cl2 (g) + 3H2O...
What are the oxidation and reduction half reactions for: 2Fe(NH4)2(SO4)2·6H2O + 3H2C2O4 + 3K2C2O4 + H2O2 → 2K3Fe(C2O4)3·3H2O + 2(NH4)2SO4 + 2H2SO4 + 8H2O
What is the half oxidation reactions( in disinfection process) for : S-2 that give after oxidation SO4-2 N that give after oxidation NO3-1
4. Which of the following reactions involves neither oxidation nor reduction? a. N2(g) + 3H2(g) - 2NH3(8) b. NH.NO(s) - N2(g) + 2H2O(1) c. Cu(s) + 2Ag (aq) → Cu²+(aq) + 2Ag(s) d. 2 Cro. (aq) + 2H*(ag) - Cr2O72- (aq) + H:0() e. CH:(8) + H2(g) - CH (8) 5. The oxidation number of nitrogen given for all the following species is correct except a. NH4 (-2). b. N30 (+1). c. NH2OH (-1). d. HNO, (+3). e. HN; (-1)....
For each of the following unbalanced half-reactions, determine whether an oxidation or reduction is occurring: 1) Mn2+ ⟶ MnO2 2) NO3 − ⟶ NO the answer for 1 is and for b is so I want to know for b how the oxidation state on Mn was +4? and for d how you the oxidation state on N was +5 and then +2? please I need the answeras soon as possible b) Mn2+→MnO2 The balanced half reaction is as follows:...
Write balanced equations for the following oxidation-reduction reactions. Show your work. a. The oxidation of Zn by MnO4- in an acidic solution to form Zn^2+ and MnO2 b. The oxidation of NO2 by Au^3+ in basic solution to form Au and NO3-
6:18 17.2 Acidic Redox Reactions to balance hydrogen content Transcript Content attribution Balance acidic oxidation-reduction reactions Question Balance the following unbalanced oxidation- reduction reaction in acidic solution: 1,(aq) + NO3(g) — 103(aq) + NO (9) Provide your answer below: 1,(aq) + H+ (aq) + NO3(aq) + 10 MORE INSTRUCTION SUBMIT Content attribution
5.012g of Fe(NH4)2(SO4)4. 6H2O Find the mass of K3[Fe(C2O4)3]·3H2O in g Fe(NH4)2(SO4)4. 6H2O + H2C2O4=FeC2O4(s) + H2SO4 + (NH4)2SO4 + 6H2O(l) FeC2O4 +K2C2O4 + H2O= Fe(OH)3(s) + .....etc Fe(OH)3 + H2O2 + K2C2O4=K3[Fe(C2O4)3]·3H2O + ..etc
Which of the following examples are oxidation-reduction reactions? Select all that are True. 0 CaCO3 + CaO + CO2 302 → 203 [CO(NH3)6]2+ + 2C1- → [CO(NH3)4Cl2] + 2NH3 Fe2+ + 2OH- → Fe(OH)2 2CH3CH2OH + O2 → 2CH3CO2H + 2H2 NH3 + HCl → NH4CI 2Fe2+ + H2O2 → 2Fe3+ + 2OH- 2[Fe(C204)313- → 2Fe(C204) + 2002 + 3C2042- Submit Answer Tries 0/4
5. (12 points) For the following oxidation reduction reaction: Zn(s)+NO3 (aq) > Zn2*(aq) + N2(g) + H20 a. What are the oxidation numbers of the reactants and products? Oxidation Number in products Element Oxidation Number in reactants Zn N b. Write the balanced oxidation half-reaction and the reduction half-reaction. (in acid medium) Balanced oxidation half-reaction: Balanced reduction half-reaction: Write the balanced full reaction c.
In addition to mass balance, oxidation-reduction reactions must be balanced such that the number of electrons lost in the oxidation equals the number of electrons gained in the reduction. This balancing can be done by two methods: the half-reaction method or the oxidation number method. The half-reaction method balances the electrons lost in the oxidation half-reaction with the electrons gained in the reduction half-reaction. In either method H2O(l), OH?(aq), and H+(aq) may be added to complete the mass balance. Which...