University:
Carleton College
Course:
CHEM 122 | Introduction to Chemistry
Academic year:

2022
Views:

405

Pages:

16
Author:

5CelestialChronicle

Balance each of the following equations. 1. 2H₂ + O₂ → 2H₂O 2. CH₄ + 2O₂ → CO₂ + 2H₂O 3. 2Na + 2H₂O → 2NaOH + H₂ 4. 2K + I₂ → 2KI 5. 2C + O₂ → 2CO 6. Zn + 2HCl → ZnCl₂ + H₂ 7. N₂ + 3H₂ → 2NH₃ 8. 2H₂O₂ → 2H₂O + O₂ 9. Fe₂O₃ + 6HCl → 2FeCl₃ + 3H₂O 10. H₂ + Br₂ → 2HBr 11. 2KNO₃ → 2KNO₂ + O₂ 12. CaBr₂ + H₂SO₄ → CaSO₄ + 2HBr 13. C₁₂H₂₂O₁₁ + 12O₂ → 12CO₂ + 11H₂O 14. H₂O + SO₃ → H₂SO₄ 15. 2HCl + CaCO₃ → CO₂ + H₂O + CaCl₂ 16. NH₃ + HCl → NH₄Cl 17. 2Al + 6HCl → 2AlCl₃ + 3H₂ 18. 3Mg + 2H₃PO₄ → Mg₃(PO₄)₂ + 3H₂ 19. Cu + 2AgNO₃ → 2Ag + Cu(NO₃)₂ 20. Ca + Pb(NO₃)₂ → Pb + Ca(NO₃)₂ 21. 2Al + 3Pb(NO₃)₂ → 2Al(NO₃)₃ + 3Pb 22. 2Zn + Sn(NO₃)₄ → 2Zn(NO₃)₂ + Sn 23. 3Cl₂ + 2Al → 2AlCl₃ 24. Br₂ + 2CuI → 2CuBr + I₂ 25. 3NH₄OH + FeCl₃ → 3NH₄Cl + Fe(OH)₃ 26. 2KBr + Pb(NO₃)₂ → 2KNO₃ + PbBr₂ 27. 2AlCl₃ + 3H₂SO₄ → Al₂(SO₄)₃ + 6HCl 28. Al₂(SO₄)₃ + 3BaCl₂ → 3BaSO₄ + 2AlCl₃ 29. Na₂CO₃ + CaCl₂ → CaCO₃ + 2NaCl 30. 2C₂H₆O + 13O₂ → 8CO₂ + 10H₂O 7. Write balanced molecular, ionic, and net ionic equations for the following double replacement reactions a. CdCl₂ + H₂S → CdS + 2HCl b. Fe(NO₃)₃ + 3LiOH → Fe(OH)₃ + 3LiNO₃ c. BaCl₂ + H₃PO₄ → Ba₃(PO₄)₂ + 6HCl 8. Write a balanced equation for each of the following acid-base neutralization reactions a. 3H₂SO₄ + 2Al(OH)₃ → 6H₂O(l) + Al₂(SO₄)₃(aq) b. 2HI + Mg(OH)₂ → 2H₂O(l) + MgI₂(aq) 9. Balance each of these equations. Identify each as to type. a. 6HCl + Fe₂O₃ → 2FeCl₃ + 3H₂O (DR) b. 4Al + 3O₂ → 2Al₂O₃ (S) c. MgCO₃ → MgO + CO₂ (D) d. HNO₃ + RbOH → RbNO₃ + H₂O (DR (A/B)) e. CH₄ + 2O₂ → CO₂ + 2H₂O (C) f. KClO₃ → KCl + 2O₂ (D) g. 2AgNO₃ + H₂S → Ag₂S + 2HNO₃ (DR) h. Cl₂ + 2KI → 2KCl + I₂ (SR) i. FeCl₃ + 3NaOH → Fe(OH)₃ + 3NaCl (DR) CHEMICAL REACTIONS - SET II 1. Write balanced molecular, ionic, and net ionic equations for the following double displacement reactions: (Make sure the products of the molecular equations are electrically neutral.) (a) Cu(NO₃)₂(aq) + 2NaOH(aq) → Cu(OH)₂(s) + 2NaNO₃(aq) (b) HgCl₂(aq) + K₂PO₄(aq) → Hg₃(PO₄)₂(s) + 2KCl(aq) (c) CaSO₄(aq) + Li₂CO₃(aq) → CaCO₃(s) + Li₂SO₄(aq) 2. Write the formulas for the following ionic compounds: magnesium phosphate: Mg₃(PO₄)₂ sodium sulfide: Na₂S copper (II) iodide: CuI₂ 3. Identify the cation and anion in each of the following aqueous solutions: (NH₄)₂CO₃: 2NH₄⁺ and CO₃²⁻ CaBr₂: Ca²⁺ and 2Br⁻ Ag₂S: 2Ag⁺ and S²⁻ 4. Using your activity series, list three metals that: (a) can be displaced by Cr: Co, Ni, Sn (b) can not be displaced by Cr: Zn, Mn, Al 5. When one metal displaces another metal, what is taking place at the atomic level? Electrons are transferred from the free metal to the metal ion in solution. 6. List three metals that will lose electrons to the Fe²⁺ ion: Ca, Na, Mg 7. Write molecular, ionic and net ionic equations for the following single displacement reactions: (a) Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s) (b) Fe(s) + Ni(NO₃)₂(aq) → Fe(NO₃)₂(aq) + Ni(s) (c) CaSO₄(aq) + Li₂CO₃(aq) → CaCO₃(s) + Li₂SO₄(aq)

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