1. Chapter 11 Test Review

2. Balance the following equation so that there are the same number of atoms on each side of the yield sign. Click on the answer box to reveal the answer. What numbers should be added to the equation, if any? Write them in the spaces below.
__CaCO __CaO + __CO2
Answer
CaCO3 CaO + CO2

3. __C + __Cl2 __CCl4 Balance the following equation. Answer

4. __NaH2PO4 __NaPO3 + ___H2O Balance the following equation. Answer
1, 1, 1

5. __H2 + __Cl2 __HCl Balance the following equation. Answer

6. Balance the following equation.
__Na + __F __NaF
Answer
2Na + F NaF

7. __H2O2 __H2O + __O2 Balance the following equation. Answer

8. __KClO3 __KCl + __O2 Balance the following equation. Answer

9. __P + __O2 __P4O10 Balance the following equation. Answer

10. ___KMnO4 + ___HCl ___KCl + ___MnCl2 + ___H2O + ___Cl2
Balance the following equation.
___KCl + ___MnCl2 + ___H2O + ___Cl2
___KMnO4 + ___HCl
Answer
2, ,2,8,5

11. ___H2SO4 + ___V2O3 ___V2(SO4)3 + ___H2O
Balance the following equation.
___H2SO4 + ___V2O3
___V2(SO4)3 + ___H2O
Answer
3, ,3

12. ___SO2 + ___H2O ___H2S + ___O2 Balance the following equation. Answer
10, ,1

13. __BaCl2 + __H2SO4 __BaSO4 + __HCl
Balance the following equation.
__BaCl2 + __H2SO __BaSO4 + __HCl
Answer
BaCl2 + H2SO BaSO4 + 2HCl

14. Balance the following equation.
__N2 + __H __NH3
Answer
N2 + 3H NH3

15. __Na + __Cl2 __NaCl Balance the following equation. Answer

16. Word Match the word with its definition. Definition reactant
a representation of a chemical reaction showing the relative numbers of reactant and product molecules
a number written before a chemical formula to represent the relative numbers of the molecule
a substance resulting from a chemical reaction
a process in which one or more substances are changed into one or more new substances by the reorganization of component atoms
the starting substance in a chemical reaction
reactant
coefficient
chemical
equation
chemical
reaction
product

17. The formula HCl stands for ____.
hydrochloric acid

18. ____ measures how acidic or basic a substance is.2
____ measures how acidic or basic a substance is. pH

19. 3
What type of reaction is shown in the following chemical equation: 2H2O ® 2H2 + O2?
decomposition

20. 4
According to the law of conservation of mass, if two atoms of hydrogen are
used as a reactant, how many atoms of hydrogen must be part of the product? 2

21. 5
According to the law of conservation of mass, how does the
mass of the products in a chemical reaction compare to the mass of the reactants?
The masses are equal.

22. 6
Numbers that precede symbols and formulas in a chemical equation are ____.
coefficients

23. synthesis What type of reaction is shown in the following7
What type of reaction is shown in the following
chemical equation: NH3 + HCl ® NH4Cl?
synthesis

24. Each substance on the left side of the arrow in a chemical equation is a ____.
reactant

25. balanced A(n) ____ chemical equation has the same number of9
A(n) ____ chemical equation has the same number of
atoms of each element on each side of the equation.
balanced

26. __Fe + __O2 __Fe2O3 Balance the following equation. Answer

27. Word
Description
Type of reaction where we have more products than reactants (numerically wise)
Type of reaction where two things are added, giving us one product.
Type of reaction where we need to use our metal activity series...only reaction where there can be no reaction.
Type of reaction that characterizes burning.
Most common type of chemical reaction.
Synthesis
Combustion
Double Replacement
Decomposition
Single Replacement

28. Write this chemical equation in word form:
Cu(s) + 2 H2O(l)
Cu(OH)2(aq) + H2(g)

29. Write this chemical equation in word form:
CO(g) + SO3
CO2(g) + SO2(g)

30. ·Write the molecular, total ionic, and net ionic equations for this reaction: Silver nitrate reacts with Lead (II) Chloride in hot water.
·(Remember your (aq), (l), & (s) symbols because those can make a difference in the net ionic equation.)

31. Molecular Equation: 2AgNO3(aq) + PbCl2(aq) = 2AgCl + Pb(NO3)2
Total Ionic Equation: 2Ag(s) + 2NO3 (aq) + PbCl2(aq) = 2AgCl + Pb(s) + 2NO3 (aq)
Net Ionic Equation: 2Ag(s) + PbCl2(aq) = 2AgCl + Pb(s)

32. Write the molecular, total ionic, and net ionic equations for this reaction: CaCO3(s) + HCl
One of the the products in this is H2CO3 which then decomposes to CO2 and liquid water...use these two products in your equations.

33. Molecular Equation: CaCO3(s) + 2HCl(aq) = CaCl2(aq) + H2O(l) + CO2(g)
Total Ionic Equation: CaCO3(s) + 2H+(aq) + 2Cl-(aq) = Ca2+(aq) + 2Cl-(aq) + H2O(l) + CO2(g)
Net Ionic Equation: CaCO3(s) + 2H+(aq) = Ca2+(aq) + H2O(l) + CO2(g)

34. Write the molecular, total ionic, and net ionic equations for this reaction: Fe(s) + AgNO3

35. Molecular Equation: Fe(s) + 2AgNO3(aq) = 2Ag(s) + Fe(NO3)2(aq)
Total Ionic Equation: Fe(s) + 2Ag+(aq) + 2NO3-(aq) = 2Ag(s) + Fe2+(aq) + 2NO3-(aq)
Net Ionic Equation: Fe(s) + 2Ag+(aq) = 2Ag(s) + Fe2+(aq)

36. What type of reaction is the following:
H2 + O2

37. What type of reaction is the following:
KBr + Cl2

38. What type of reaction is the following:
Zn + H2SO4

39. What type of reaction is the following:
C4H10 + O2

40. What type of reaction is the following:
HgO

41. What type of reaction is the following:
AgNO3 + NaCl

42. What type of reaction is the following:
C8H8 + O2

43. What type of reaction is the following:
Mg(OH)2 + H2SO3