Test 3 Practice - briggs225

93 downloads 920 Views 123KB Size Report
Practice Test #3. ____ 1. When a precipitation reaction ... All of the following are clues that a chemical reaction has taken place except. A) A color change occurs.
Name: ___________________________________ Date: ______________

Practice Test #3 ____

1. When a precipitation reaction occurs, the ions that do not form the precipitate A) evaporate B) are cations only C) form a second insoluble compound in the solution D) are left dissolved in the solution E) none of these

____

2. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E)

____

3. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The net ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E) No net ionic equation exists for this reaction.

____

4. All of the following are clues that a chemical reaction has taken place except A) A color change occurs. D) Bubbles form. B) A solid forms. E) A flame occurs. C) The reactant is smaller.

____

5. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? Al + Fe3 O4 A) 1

____

Al2 O3 + Fe B) 3

C) 6

D) 9

E) 12

6. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? CH3 OH + O2 A) 1

CO2 + H2 O B) 2

C) 3

D) 4

E) 6

____

7. Which of the following statments is not true of balancing a chemical equation? A) Subscripts in the reactants must be conserved in the products. B) Coefficients are used to balance the atoms on both sides. C) The law of conservation of matter must be followed. D) Phases are often shown for each compound but are not critical to balancing an equation. E) All of the above statements (a-d) are true.

____

8. Which of the following statments is not true of balancing a chemical equation? A) Subscripts in the reactants must be conserved in the products. B) Coefficients are used to balance the atoms on both sides. C) The law of conservation of matter must be followed. D) Phases are often shown for each compound but are not critical to balancing an equation. E) All of the above statements (a-d) are true.

____

9. The factors that most commonly cause chemical reactions to occur are all the following except A) formation of a solid D) transfer of electrons B) formation of a gas E) a decrease in temperature C) formation of water

____ 10. An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead(II) nitrate. Identify the solid in the balanced equation. A) (NH4 )2 SO4 B) Pb(NO3 )2 C) PbSO4 D) NH4 NO3 E) There is no solid formed when the two solutions are mixed. ____ 11. An aqueous solution of sodium carbonate is reacted with an aqueous solution of calcium chloride. Identify the solid in the balanced equation. A) Na2 CO3 B) CaCl2 C) NaCl D) CaCO3 E) There is no solid formed when the two solutions are mixed. ____ 12. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. Identify the solid in the balanced equation. A) KCl B) NaNO3 C) KNO3 D) NaCl E) There is no solid formed when the two solutions are mixed.

____ 13. An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead(II) nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E) ____ 14. An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead(II) nitrate. The net ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E) ____ 15. True or false? The complete ionic equation contains only those substances directly involved in reactions in aqueous solutions. A) True B) False 16. Balance the equation NaBH4 + BF3 → NaBF4 + B2 H6 17. Balance the equation Mg(OH)2 (aq) + HBr(aq) → MgBr2 (aq) + H2 O(l) 18. Balance the equation Sb(s) + O2 (g) → Sb2 O3 (s) 19. Balance the equation for the reaction of potassium metal with water to form potassium hydroxide and hydrogen gas. 20. Balance the equation for the reaction of aluminum metal with solid iodine to form solid aluminum iodide. 21. Balance the equation HCl(aq) + Ca(OH)2 (aq) → CaCl2 (aq) + H2 O(l) 22. Balance the equation Fe(NO3 )2 (aq) + H2 S(g) → FeS(s) + HNO3 (aq) Use the following to answer questions 23-24. Write and balance molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and phases of the products in each of the cases. 23. An aqueous solution of barium nitrate is mixed with an aqueous solution of potassium phosphate. 24. An aqueous solution of silver nitrate is mixed with an aqueous solution of potassium chromate.

25. Write the balanced molecular equation for the reaction between aqueous solutions of lithium phosphate and sodium hydroxide. Use the following to answer questions 26-35. Use the following choices to classify each reaction given below (more than one choice may apply). S. synthesis D. decomposition SR. single replacement DR. double replacement C. combustion OR. oxidation-reduction AB. acid-base P. precipitation 26. ZnBr2 (aq) + 2AgNO3 (aq) → Zn(NO3 )2 (aq) + 2AgBr(s) 27. KBr(aq) + AgNO3 (aq) → AgBr(s) + KNO3 (aq) 28. HNO3 (aq) + NaOH(aq) → H2 O(l) + NaNO3 (aq) 29. H2 SO4 (aq) + Ba(OH)2 (aq) → 2H2 O(l) + BaSO4 (s) 30. Zr(s) + O2 (g) → ZrO2 (s) 31. Zn(s) + 2HCl(aq) → H2 (g) + ZnCl2 (aq) 32. 6Na(s) + N2 (g) → 2Na3 N(s) 33. Na2 SO4 (aq) + Pb(NO3 )2 (aq) → PbSO4 (s) + 2NaNO3 (aq) 34. 2HCl(aq) + Pb(OH)2 (aq) → PbCl2 (s) + 2H2 O(l) 35. 2Hg(l) + O2 (g) → 2HgO(s) 36. 2HgO(s) → 2Hg(l) + O2 (g) 37. 2Na(s) + H2 (g) → 2NaH(s) 38. C(s) + O2 (g) → CO2 (g) 39. 2Cs(s) + F2 (g) → 2CsF(s)

40. C3 H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2 O(g) 41. 2H2 O(l) → 2H2 (g) + O2 (g) 42. S8 (s) + 12O2 (g) → 8SO3 (g) 43. P4 (s) + 5O2 (g) → P4 O1 0(s) 44. 2GaN(s) → 2Ga(s) + N2 (g)

Answer Key - Test 3 Practice 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44.

D C E C D D A A E C D E B D False 3NaBH4 + 4BF3 → 3NaBF4 + 2B2 H6 Mg(OH)2 (aq) + 2HBr(aq) → MgBr2 (aq) + 2H2 O(l) 4Sb(s) + 3O2 (g) → 2Sb2 O3 (s) 2K(s) + H2 O(l) → 2KOH(aq) + H2 (g) 2Al(s) + 3I2 (s) → 2AlI3 (s) 2HCl(aq) + Ca(OH)2 (aq) → CaCl2 (aq) + 2H2 O(l) Fe(NO3 )2 (aq) + H2 S(g) → FeS(s) + 2HNO3 (aq) 3Ba(NO3 )2 (aq) + 2K3 PO4 (aq) → Ba3 (PO4 )2 (s) + 6KNO3 (aq) 2AgNO3 (aq) + K2 CrO4 (aq) → Ag2 CrO4 (s) + 2KNO3 (aq) Li3 PO4 (aq) + 2NaOH(aq) → Na3 PO4 (aq) + 3LiOH(aq) DR DR, P DR, AB DR, AB, P S, OR SR, OR S, OR DR, P DR, P S, C, OR D, OR S, OR S, OR, C S, OR C, OR D, OR S, OR, C S, OR, C D, OR