Numbers 8, 9 and 10 only Direction: Write the oxidation half-reaction and reduction half-reaction, and shorthandelectrochemical notation for the following.1. Mg + H+ → Mg2+ + H₂2. KI + Cl₂ →→→ KCl + I₂3. Cr+ + Sn4+ → Cr³+ + Sn²+4. 3 Hg₂+ + 2 Fe (s) → 3 Hg2+2 Fe³+5.2 As (s) + 3 Cl2 (g) → 2 AsCl36. NaBr + Cl₂ → NaCl + Br27. Fe2O3 + CO → Fe + CO28. CO + I205 → CO₂ + I29. 2 Fe ³+ (aq) + Sn²+ (aq) → 2 Fe ²+ + Sn¹+ (aq)10. Chlorine gas oxidises Fe 2+ ions to Fe³+ ions. In the process, chlorine is reduced tochloride ions.

Oxidation means loss of electrons and reduction means gain of electrons.

Direction: Write the oxidation half-reaction and reduction half-reaction, and shorthand electrochemical notation for the following. 1. Mg + H+ → Mg2+ + H₂ 2. KI + Cl₂ KCl + 1₂ 3. Cr+ + Sn4+ → Cr³+ + Sn²+ 4. 3 Hg₂+ + 2 Fe (s) - 3 Hg₂+2 Fe³+ 5.2 As (s) + 3 Cl₂ (g) → 2 AsCl3 6. NaBr + Cl₂ → NaCl + Br2 7. Fe2O3 + CO → Fe + CO₂ 8. CO + 1₂05 CO₂ + I₂ 3+ 9.2 Fe ³+ (aq) + Sn²+ (aq) → 2 Fe ²+ + Snª*(aq) 2+ ions to Fe³+ ions. In the process, chlorine is reduced to 10. Chlorine gas oxidises Fe chloride ions.

Direction: Write the oxidation half-reaction and reduction half-reaction, and shorthand electrochemical notation for the following. 1. Mg + H+ → Mg2+ + H₂ 2. KI + Cl₂ KCl + 1₂ 3. Cr+ + Sn4+ → Cr³+ + Sn²+ 4. 3 Hg₂+ + 2 Fe (s) - 3 Hg₂+2 Fe³+ 5.2 As (s) + 3 Cl₂ (g) → 2 AsCl3 6. NaBr + Cl₂ → NaCl + Br2 7. Fe2O3 + CO → Fe + CO₂ 8. CO + 1₂05 CO₂ + I₂ 3+ 9.2 Fe ³+ (aq) + Sn²+ (aq) → 2 Fe ²+ + Snª*(aq) 2+ ions to Fe³+ ions. In the process, chlorine is reduced to 10. Chlorine gas oxidises Fe chloride ions.

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...

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