1. Synthesis of triacetylacetonatomanganate(III), [Mn(CH3COCH2COCH3)3] or [Mn(acac)3]
Write half and overall redox equations for the following reaction.
MnO2 + 5Mn2+ + 8H+ -----> 6Mn3+ + 4H2O
Mn3+ + 3CH3COCH2COCH3 + 3OH- -------> [Mn(CH3COCH2COCH3)3] + 3H2O
1. Synthesis of triacetylacetonatomanganate(III), [Mn(CH3COCH2COCH3)3] or [Mn(acac)3] Write half and overall redox equations for the following...
Write balanced half-reactions for the following redox reaction: 512(3)+2 Mn²+ (aq)+160H (aq) → 101 (aq)+2 MnO2 (aq)+8 H20(1) reduction: oxidation:
Write the half-reactions and the net ionic equations for these complete redox reactions 4 2NaCl (aq) + Br: (I) Cl: (g)2NaBr (aq) a) Oxidation half-reaction: Reduction half-reaction: CrCls (aq)+ Au (s) AuCl3(aq) Cr (s) - b) Oxidation half-reaction: Reduction half-reaction: Identify the oxidizing agent and the reducing agent in these complete redox reactions: 5. 5SO2-2Mn2+ 5so +3H2O a) 2MnO, +6H A) MnO B) So2 C) Mn2 D) SO E) H Oxidizing agent: b) 5Fe2 (aq) + MnO4 (ag) +8H'(aq)-5Fe (ag)+...
Question 3 Write the balanced half-reaction for the reduction of permanganate ion to Mn- in an acidic solution MnO4 (aq) +SH+ (aq) + 5e Mn2-(aq) + 4H2O(1) MnO, (aq) + 4H+ (aq) - 31 --Mn-(ag) - 40H(aq) MnO4 (aq) + 5e – Mn"(aq) + 202(g) MnO,- (aq) - 8H+ (aq) — Mn2+(ag) - 4H2O() Mno"(aq) + 4H+ (aq) - 5e – Mn?-(aq) - 40H(aq)
Write balanced half-reactions for the following redox reaction: MnO4^-(aq) + 4H2O(l) + 5Cu^+(aq) = Mn^2+(g) + 8OH^-(aq) +5Cu^2+(aq)
3. Calculate the redox potential (in volts) for a LiMnO2/graphite battery. (Redox reaction) MnO4- + 8H + 5e- → Mn2+ (aq) + 4H2O (+1.51 V) MnO2 + 4H +2e- → Mn2+ (aq) + 2H2O (+1.22 V) xLi+ + C6 + e- → LixC5 (-3.00 V) 1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f....
Write a balanced equation for the following synthesis. (No other reactants were used) a) synthesis of [Mn(acac)3] / reactants: KMnO4, H2O, and acytylacetone b) synthesis of [Cr(acac)3] / reactants: chromium(III) chloride hexahydrate, urea, H2O, and acytylacetone
3. Calculate the redox potential (in volts) for a LiMnO2/graphite battery. MnO4- + 8H + 5e- → Mn2+ (aq) + 4H2O (+1.51 V) MnO2 + 4H +2e- → Mn2+ (aq) + 2H2O (+1.22 V) xLi+ + C6 + e- → LixC5 (-3.00 V) 1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f. The reaction...
please help 11. Disproportionation a. Consider the following reaction. 3Ch 5CL + Cls. Write two balanced half equations (one oxidation, one reduction) to show the changes that the chlorine species undergoes. OXIDATION: REDUCTION: b. Is this reaction a disproportionation? Justify your answer. 12. REDOX Titration calculations a. Consider the following half equations. SO32- + H2O + SO42- + 2H+ + 2e. MnO4- + 8H. + 5e- → Mna: + 4H2O Combine these two equations to obtain the overall reaction of...
use the half reaction method to balance (SHOW ALL WORK) the following overall redox reaction describing the formation of acid mine drainage emanating from coal mines FeS2(s)+o2(g)+H2o(l)->FE(OH)3(s) +SO4 2-(aq) +H+(aq) balance redox entirely 1)FeS2+o2+h2o->fe2+ +So4 2- +h+ Balance redox entirely 2)2Fe2+ . + 1/2 O2 + 2H+ . ->2Fe3+ +H20 Balance this precipitation reaction Fe3+(aq) +3H2o(l) . -> F(OH)3 (s) +3H+(aq)
Which of the reactions involving metal ions (Equations 1A – 6B ) represent redox reaction(s)? Write down the entire equation(s) AS WELL AS their corresponding balanced oxidation half-reaction(s) AND reduction half-reaction(s). Ag+(aq)+ HCl(aq)+ H2O(l) -> AgCl(s, white)+ H3O+(aq) Eq. 1A AgCl(s)+ 2NH3(aq) -> [Ag(NH3)2]+(aq)+ Cl–(aq) Eq. 2A Fe3+(aq)+ 3NH3(aq)+ 3H2O(l) -> Fe(OH)3(s)+ 3NH4(aq) Eq. 3A Fe3+(aq)+ 6SCN–(aq) -> Fe(SCN)63–(aq, blood-red) Eq. 4A Co2+(aq)+ 7NO2–(aq)+ 3K+(aq)+ 2H3O+(aq) -> NO(g)+ 3H2O(l)+ K3[Co(NO2)6](s, yellow) Eq. 6A 2 NO(g, colorless)+ O2(g) →2NO2(g, red-brown) Eq....