**Electron-Transfer Reactions Tutorial**For the following electron-transfer reaction:$$3\text{Ni}^{2+}(\text{aq}) + 2\text{Al}(\text{s}) \rightarrow 3\text{Ni}(\text{s}) + 2\text{Al}^{3+}(\text{aq})$$You are required to enter the electrons as $ e^- $.**Important Guidance:**Use the smallest possible integer coefficients.If a box is not needed, leave it blank.**Tasks:**1. **Oxidation Half-Reaction:** Fill in the boxes to balance the oxidation half-reaction. \[\boxed{} \; + \; \boxed{} \; \rightarrow \; \boxed{} \; + \; \boxed{\boxed{\text{Al}^{3+}}} \; + \; \boxed{}\] 2. **Reduction Half-Reaction:** Fill in the boxes to balance the reduction half-reaction. \[\boxed{} \; + \; \boxed{}\; e^- \rightarrow \; \boxed{} \; + \; \boxed{\boxed{\text{Ni}^{2+}}} \; + \; \boxed{}\] Each reaction must be balanced by ensuring the same number of each type of atom on both sides of the equation and by balancing the charges with the appropriate number of electrons.

Concept Introduction: Lose of electron oxidation (LEO) Gain of…

Science

Chemistry

3Ni*(aq) + 2Al(s) 3Ni(s) + 2A*(aq) The oxidation half-reaction is:

3Ni(aq) + 2Al(s) 3Ni(s) + 2A(aq) The oxidation half-reaction is:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Balance each redox reaction occurring in acidic aque- ous solution. Use the half-reaction method. (a) Cl0, (aq) + CI^(aq) –→ CIO3 (aq) + Cl2(g) (b) MnO4¯(aq) + Al(s) → Mn²*(aq) + Al³*(aq) (c) Br2(aq) + Sn(s) → Sn2*(aq) + Br¯(aq)
Aqua regia, a mixture of concentrated HNO3 and HCl, was developed by alchemists to “dissolve” gold. The process is a redox reaction with the following simplified skeleton reaction: Au(s) + NO3- (aq) + Cl- (aq) AuCl-4 (aq) + NO2 (g) (a) Balance the reaction by the half- reaction method (b) What is the oxidizing and reducing agents? (c) What is the function of HCl in aqua regia?
41. Balance each of the following equations according to the half-reaction method: (a) MnO4 (aq) + NO2 (aq) →→MnO2 (s) + NO3(aq) (in base) (b) MnO2 (aq)MnO4 (aq) + MnO2(s) (in base) (c) Br2(l) + SO2(g) → Br¯(aq) + SO4² (aq) (in acid)
Write a balanced net ionic equation for a redox reaction that results in the formation of potassium chloride. (Assume that potassium chloride is not a starting material, and assume the reaction takes place in aqueous solution.) X, Не (aq), 2K(ag)+Cl, (aq) KCI(aq)
balance the following redox reaction if it occurs in basic solution. what are the coefficients in front of CLO2 and H2O in the balanced reaction? H2O2(1) + ClO2 (aq) --> ClO2- (aq) + O2(g)
Write a balanced equation for the following redox reaction in abasic solutionVO2+(aq) + NO(g) → V3+(aq) + NO2(g)
Balance the following oxidation-reduction reaction that occurs in an acidic solution using the half-reaction method. |(aq) + ClO"(aq) → 13 (aq) + Cl¯(aq) HOW DO WE GET THERE? Which half-reaction correctly uses electrons to balance the charge? 31 (aq) → 13 (aq) + 1e- 3e +31"(aq) → I3 (aq) 2e +31"(aq) → I3 (aq) 31 (aq) → 13 (aq) + 2e¯ 31 (aq) → 13 (aq) + 3e- Check Next (3 of 6)
Write balanced half-reactions for the following redox reaction: 2+ 2+ 3+ MnO4(aq) +8 H* (aq) +5 Fe²+ (aq) Mn²+ (aq) + 4H₂O(1)+5 Fe³+ (aq)
Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Cl2 and OH- in the balanced reaction?Cl2(g) → ClO3-(aq) + Cl-(aq)
Classify each half-reaction as a reduction or an oxidation. 10⁰00 Cr₂O² (aq) + 14 H+ (aq) + 6 e¯ → 2 Cr³ ¹(aq) + 7 H₂O(1) Fe³+ (aq) + 3 e - Fe(s) Au(s) + 2 CN (aq) - → Au(CN)₂ (aq) + e¯ HgO(s) + H₂O(1) + 2 e¯ → Hg(1) + 2 OH (aq) 2 CI (aq) → Cl₂(g) + 2 e Answer Bank oxidation reduction
Balance the net ionic redox equation by the half-reaction method, in acid and in base: __Fe(s) + __ClO4 ̄(aq) __Fe3+(aq) + __Cl ̄(aq)
Write balanced half-reactions for the following redox reaction: 2 CO₂(g) +12H* (aq) +6C₂0 (aq) → C₂H₂OH()+ 3 H₂O(1)+12 CO₂(aq)