Write balanced half-reactions for the following redox reaction: 8Fe+3(aq)+AsH3(g)+4H2O(l)? 8Fe+2(aq)+H3AsO4(aq)+8H+(aq) I think red: 8Fe3+?8Fe2+(aq)+e- ox: 8e-...

Write balanced half-reactions for the following redox reaction:

8Fe+3(aq)+AsH3(g)+4H2O(l)? 8Fe+2(aq)+H3AsO4(aq)+8H+(aq)

I think red: 8Fe3+?8Fe2+(aq)+e- ox: 8e- + AsH3(g)+4H2O(l)?H3AsO4(aq)+8H+(aq) just need some calification please :)

Expert Solution

queen_honey_blossom answered 3 years ago

Write balanced half-reactions for the following redox reaction: 2CO2(g)+9H2O(l)+12Fe+2(aq)→ C2H5OH(l)+12OH−(aq)+12Fe+3(aq)

1. a) Show the balanced half reactions and the total balanced reaction for the following redox...

1. a) Show the balanced half reactions and the total balanced reaction for the following redox reaction in acidic solution. RuO4 + H2SeO3 → Ru3+ + SeO42- b) Comment on whether you expect this reaction to be spontaneous. Show all of your work.b 2 (a) Use the Lattimer diagram for chlorine in basic conditions to determine the potential for reduction of ClO4- to Cl2 . (b) Write a balanced equation for this half reaction

Problem 20.51 Given the following reduction half-reactions: Fe3+(aq)+e??Fe2+(aq) E?red=+0.77V S2O2?6(aq)+4H+(aq)+2e??2H2SO3(aq) E?red=+0.60V N2O(g)+2H+(aq)+2e??N2(g)+H2O(l) E?red=?1.77V VO+2(aq)+2H+(aq)+e??VO2+(aq)+H2O(l) E?red=+1.00V Part...

Problem 20.51 Given the following reduction half-reactions: Fe3+(aq)+e??Fe2+(aq) E?red=+0.77V S2O2?6(aq)+4H+(aq)+2e??2H2SO3(aq) E?red=+0.60V N2O(g)+2H+(aq)+2e??N2(g)+H2O(l) E?red=?1.77V VO+2(aq)+2H+(aq)+e??VO2+(aq)+H2O(l) E?red=+1.00V Part A Write balanced chemical equation for the oxidation of Fe2+(aq) by S2O2?6 (aq). Express your answer as a chemical equation. Identify all of the phases in your answer. SubmitMy AnswersGive Up Part B Calculate ?G? for this reaction at 298 K. Express your answer using two significant figures. ?G? = kJ SubmitMy AnswersGive Up Part C Calculate the equilibrium constant K for this reaction...

Balance the following redox reactions. Show the complete balanced reduction half and oxidation half reaction, and...

Balance the following redox reactions. Show the complete balanced reduction half and oxidation half reaction, and label each accordingly. Give the complete balanced reaction. A.) CN-1 + MnO4-2 ---> CNO-1 + MnO2 B.) S2O3-2 + IO2-1 ---> I- + S4O6-2

Write the balanced half-reaction for the following redox reaction (include physical states like I did in...

Write the balanced half-reaction for the following redox reaction (include physical states like I did in final answer): 2CO2(g) + 12H+(aq) + 6Zn(s) -----> C2H5OH(l) + 3H2O(l) + 6Zn2+(aq)

Balance the following redox reactions, in base, using the half-reaction method. Clearly identify each balanced half-reaction...

Balance the following redox reactions, in base, using the half-reaction method. Clearly identify each balanced half-reaction and the overall balanced equation. C3H8O2 (a) + Cr2O72– (aq)  C3H4O4 (aq) + 2 Cr3+ (aq)

20#15 Given the following half-reactions and associated standard reduction potentials: AuBr−4(aq)+3e−→Au(s)+4Br−(aq) E∘red=−0.858V Eu3+(aq)+e−→Eu2+(aq) E∘red=−0.43V IO−(aq)+H2O(l)+2e−→I−(aq)+2OH−(aq) E∘red=+0.49V...

20#15 Given the following half-reactions and associated standard reduction potentials: AuBr−4(aq)+3e−→Au(s)+4Br−(aq) E∘red=−0.858V Eu3+(aq)+e−→Eu2+(aq) E∘red=−0.43V IO−(aq)+H2O(l)+2e−→I−(aq)+2OH−(aq) E∘red=+0.49V Sn2+(aq)+2e−→Sn(s) E∘red=−0.14V a) Write the cell reaction for the combination of these half-cell reactions that leads to the largest positive cell emf. b) Calculate the value of this emf. E∘max = _____ V c) Write the cell reaction for the combination of half-cell reactions that leads to the smallest positive cell emf. d) Calculate the value of this emf. E∘min = _____ V

An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)?Pb2+(aq, 0.21M )+2e? Red: MnO?4(aq,...

An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)?Pb2+(aq, 0.21M )+2e? Red: MnO?4(aq, 1.25M )+4H+(aq, 2.5M )+3e?? MnO2(s)+2H2O(l). Compute the cell potential at 25 ?C.

Exercise 18.62 Calculate E∘cell for each of the following balanced redox reactions. Part A O2(g)+2H2O(l)+4Ag(s)→4OH−(aq)+4Ag+(aq) Express your answer...

Exercise 18.62 Calculate E∘cell for each of the following balanced redox reactions. Part A O2(g)+2H2O(l)+4Ag(s)→4OH−(aq)+4Ag+(aq) Express your answer using two significant figures. E∘cell = V Part B Br2(l)+2I−(aq)→2Br−(aq)+I2(s) Express your answer using two significant figures. E∘cell = V Part C PbO2(s)+4H+(aq)+Sn(s)→Pb2+(aq)+2H2O(l)+Sn2+(aq) E∘cell = v

Calculate E∘cell for each of the following balanced redox reactions. Are the reactions spontanous? A) 2Cu(s)+Mn2+(aq)→2Cu+(aq)+Mn(s)...

Calculate E∘cell for each of the following balanced redox reactions. Are the reactions spontanous? A) 2Cu(s)+Mn2+(aq)→2Cu+(aq)+Mn(s) B) MnO2(s)+4H+(aq)+Zn(s)→Mn2+(aq)+2H2O(l)+Zn2+(aq) C) Cl2(g)+2F−(aq)→F2(g)+2Cl−(aq)

Question