Chem Electrolysis Practice Problems Key

University:
Cornell University
Course:
CHEM 2070 | General Chemistry I
Academic year:

2019
Views:

343

Pages:

9
Author:

layenryPypemx5

Chemistry Redox Practice name: Κεν hour: For the following substances, list the oxidation number of the Indicated element. 1. Na3PO4 Na= +1 P= +5 -2 2. CH4 C= +4 H=+1 3. K2CrO4 K=+1 Cr=+b O= -2 4. Na₂SO₄ Na +1 S= +6 0= -2 5. HBrO4 H= +1 Br= +7 0 -2 6. HBrO3 H=+1 Br= +5 0-2 7. HBrOz H= +1 Br= +3 0= -2 8. HBrO H= +1 Br= +10= -2 9. NO N=+2 0= -2 10. NO2 N= +4 0-2 11. 205 N= +5 -2 0= 13 11. C₂H₃O₂ C=OH= +10=-2 13. MnO4 Mn+70= -2 12. NaHCO3 Na=+ H=+1 C=4 0=-2 Write the reaction for the process where 15. A neutral metal atom becomes a 2+ ion M M2+ +2e 16. A4+ metal lon becomes a 2+ metal ion M4+ +2e M2+ State whether the following represents an oxidation, a reduction, or neither for the element on both sides of the arrow 17. Na NaCl Oxidized +1 18. NH, reduced 19. қою, ch reduced نام +5 br 20. CO₂CH₂ reduced Consider the reaction: PbO2 42-1 +4HI12 Pilz + 41-2 2H2O 21. Which substance is oxidized? 22. Which substance is reduced? Pb 23. Which substance is the reducing agent? HI 24. Which substance is the oxidizing agent? ELECTROCHEMICAL CELL REACTION PRACTICE Given the following reactants, write the half reactions, balance the electrons, and write the overall equations for each possible combination producing an electrochemical cell. Indicate which element or lon is oxidized and which is reduced. Then write the cell notation for each electrochemical cell, and calculate the call voltage. Given: solid Al, Ag, Mg, Zn, and Cu, and 0.1M solutions of: Al³, Ag, Mg, Zn2+, and Cu2+ Al → Al3+3e axidized = AL reduced = Ag Aqt le Ag call notation: A1/A13+-11 Ag+Ag Al + 3 AqA1B1 3A9 Ecl call 2.46 Al → Al3++30- Mq+Ze Ma 2A1+3Mq22A1B3+ + 3Mg oxidized = Al reduced = Mg2+ cll notation: A1/A13+11 MG 2 Mg E= -71 axidized= reduced = cell notation: Continue like this for the rest of the 2 pages oxidized= reduced= cell notation: Ecl oxidized = reduced= cell notation: oxidized = reduced = cell notation: Chemistry Electrochemical cell practice Calculate Es and write the half reactions and the overall cell reaction for the following: a) Al Al Cu² | Cu Al Al3+ + 3e Cu2+ +2e Cu 2A1+ 3Cu2+2A13+ + 3Cu b) Ba Ba Ag Ag Ba Ba2+ + 2e- Ag++le Ag 2Ag+ + Ba Ba2+ + 2Ag Ec-34-(-1.66) 2 c) Na Na Ni² | Ni Ecell 80-(-2.9) 3.7 Na Nat+le- Ni2+ +2e Ni 2Na+ Ni2+ 2Na+ + Ni P25-(-2.71) 12.461 d) Mg | Mgl Iz | I Mg Mq2+ +2e 12+2e21 12+ MgMq2+ +21- Ecell53-(-2.37) 2.9 (ay) ELECTROLYSIS PRACTICE QUESTIONS AND PROBLEMS Reduction always takes place at the cathode. Oxidation always takes place at the anode When an ionic compound undergoes electrolysis, the union may be oxidized, and the cation ion lon may be reduced. What is the difference between molten and aqueous? in water, molten is aqueous is dissolved a liquid swasta nice Which of the following reactions shows: a) the reduction of water b) the oxidation of water a 2H2O + 2e- →H2 + 2OH ↓ e gained E-83 2H₂O O2+4H + 4e E=123 e- 108t For the following substances, indicate which ions or molecules are present, and indicate what would be oxidized and what would be reduced. 1) AlCl3(aq) present: A13 CI, H2D + reduced: H20-1 -83 present: Ba2+, 1,20 4) FeBr2(1) 7) Balz(eq) present: Fe2+, Br oxidized: H20 1.3 1.23 oxidized: Br axidized: 53 1.28 reduoud: Fe 2 reduced: H20-29 83 5) COF2(aq) 8) Balan present: 10 F,HO Ba present: oxidized: H2O oxidized: reduced: Co2+ 6) COF2 (1) 2) AlCl3(0) present: Al3+, CI- oxidized: CI reduced: A13+ 3) FeBr2(aq) present: Fe2+ Br, Ha oxidized: B reduced: 2+ present: Co oxidized: F reduced: (024 reduced: Ba2+ 9) NaCl() present: Nat, CI- oxidized: CI reduced: Na

Chem Electrolysis Practice Problems Key

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