Balance the following half-reaction by adding the appreciate number of electrons.
Fe^2+ (aq) --> Fe^3+ (aq)
AgI(s) --> Ag(s)+I^-(aq)
VO2^+(aq)+2H^+(aq) --> VO^2+(aq)+H2O(l)
I2(s)+6H2O(l) --> 2IO3^-(aq)+12H^+(aq)
1) Fe2+(aq)------> Fe3+(aq)+ e-
2) AgI(s) + e- -----> Ag(s) + I-(aq)
3) VO2+(aq) + 2H+(aq) + e- -------> VO2+(aq) + H2O(l)
4) I2(s) + 6H2O(l) ------> 2IO3-(aq) + 12H+(aq) + 10e-
Balance the following half-reaction by adding the appreciate number of electrons. Fe^2+ (aq) --> Fe^3+ (aq)...
4.102. Balance the following half-reactions by adding the appropriate number of electrons. Which are oxidation half reactions and which are reduction half-reactions a. Fe2+ (aq) → Fe3+ (aq) b. Agi() ► Ag(s) + I (ag) c. VO,*(aq) + 2 H+ (aq) → VO2+ (aq) + HOO) d. 1() + 6 H2O(C) – 2 10,- (aq) + 12 H*(aq)
Please show all steps taken (prefer typed solution) Half-Reaction E ° (V) Ag+ (aq) + e− → Ag (s) 0.7996 Al3+ (aq) + 3e− → Al (s) −1.676 Au+ (aq) + e− → Au (s) 1.692 Au3+ (aq) + 3e− → Au (s) 1.498 Ba2+ (aq) + 2e− → Ba (s) −2.912 Br2 (l) + 2e− → 2Br− (aq) 1.066 Ca2+ (aq) + 2e− → Ca (s) −2.868 Cl2 (g) + 2e− → 2Cl− (aq) 1.35827 Co2+ (aq) + 2e−...
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.)
A galvanic cell is powered by the following redox reaction: 5Cl2 (g) + I2(s) + 6H2O(l) → 10Cl−(aq) + 2IO3-(aq) + 12H+(aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer...
Consider the following unbalanced reaction: 1035(aq) + (aq) + H+(aq) → 12(s) + H2O(1) The correctly balanced reduction half-reaction is: (A) 21+(aq) → 12(s) + 2e- (B) 2H+(aq) + 2e → H2O(1) (C) 103 (aq) + (aq) → 12(s) + 302-(aq) + 4e (D) 2103(aq) + 12H+(aq) + 10 → 12(s) + 6H2O(1) (E) 61-(aq) + 8H+(aq) + 2e → 312(s) + 4H2O(1)
please consider the reaction below Fe^2+(aq)+MnO-4(aq)>Fe^3+(aq)+Mn^2+(aq) write the oxidation half-reaction and balance write the reduction half-reaction and balance combine both half-reactions and balance
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 compound is being reduced in the following reaction: H2O2 (aq) + 2 Fe2+ (aq) + 2 H3O+ (aq) → 2 Fe3+ (aq) + 4 H20 (1) How many electrons are transferred in the following reaction? 2C103- +12H+ + 101 512 + Cl2 + 6H2O Show your work to get credit. What is the Eºcell, AG', and K for the following reaction? 12(s) + Mg(s) → Mg2+(aq) +2 1. (aq) You must show your work to get credit. Reduction Half-Reaction...
Refer to the following standard reduction half-cell potentials at 25∘C : VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V Part A Part complete An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.017M)+2H+(aq,1.3M)+e−→→Ni2+(aq,2.5M)+2e−VO2+(aq,2.5M)+H2O(l) Calculate the cell potential under these nonstandard concentrations.
Identify the Lewisacid that acts as a reactant in the following reaction Fe(H2O)63+(aq) + 6CN-(aq) →Fe(CN)63-(aq) + 6H2O(l). Fe(H2O)63+ H2O Fe3+ CN- is it the Fe3+ or the CN-,,,kinda of confused...