Adapted by Nelson Nuñez-Rodriguez
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By David W. Ball
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| QUESTION | ANSWER |
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1. Chemical equations can also be used to represent physical processes. Write a chemical reaction for the boiling of water, including the proper phase labels. |
1. H2O(ℓ) → H2O(g) |
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3. Explain why 4Na(s) + 2Cl2(g) → 4NaCl(s) should not be considered a proper chemical equation. |
3. The coefficients are not in their lowest whole-number ratio. |
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5. Does the chemical reaction represented by 3Zn(s) + 2Al(NO3)3(aq) → 3Zn(NO3)2(aq) + 2Al(s)proceed as written? Why or why not? |
5. No; zinc is lower in the activity series than aluminum. |
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7. Explain what is wrong with this double-replacement reaction. NaCl(aq) + KBr(aq) → NaK(aq) + ClBr(aq) |
7. In the products, the cation is pairing with the cation, and the anion is pairing with the anion. |
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9. Write the complete and net ionic equations for this double-replacement reaction. BaCl2(aq) + Ag2SO4(aq) → ? |
9. Complete ionic equation: Ba2+(aq) + 2Cl−(aq) + 2Ag+(aq) + SO42−(aq) → BaSO4(s) + 2AgCl(s) Net ionic equation: The net ionic equation is the same as the complete ionic equation. |
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11. Identify the spectator ions in this reaction. What is the net ionic equation? NaCl(aq) + KBr(aq) → NaBr(aq) + KCl(aq) |
11. Each ion is a spectator ion; there is no overall net ionic equation.. |
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13. Can a reaction be a composition reaction and a redox reaction at the same time? Give an example to support your answer. |
13. Yes; H2 + Cl2 → 2HCl (answers will vary) |
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15. Can a reaction be a decomposition reaction and a redox reaction at the same time? Give an example to support your answer. |
15. Yes; 2HCl → H2 + Cl2 (answers will vary) |
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17. Why is CH4 not normally considered an acid? |
17. It does not increase the H+ ion concentration; it is not a compound of H+. |
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19. What are the oxidation numbers of the nitrogen atoms in these substances?
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19.
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21. Disproportion is a type of redox reaction in which the same substance is both oxidized and reduced. Identify the element that is disproportionating and indicate the initial and final oxidation numbers of that element. 2CuCl(aq) → CuCl2(aq) + Cu(s) |
21. Copper is disproportionating. Initially, its oxidation number is +1; in the products, its oxidation numbers are +2 and 0, respectively. |