1. Write and balance chemical reactions Energy in chemical reactions
Whiteboard Review

2. Solid mercury (II) oxide breaks apart into solid mercury and oxygen gas.
Type of reaction:
Balanced Equation using (s, l, g, aq) and Energy:
Spontaneous or Non?
Exo or Endothermic?

3. Solid mercury (II) oxide breaks apart into solid mercury and oxygen gas.
Decomposition
2 HgO (s) + Energy  2 Hg (s) + O2 (g)
Nonspontaneous
Endothermic

4. Liquid dicarbon dihydride reacts with oxygen gas to form carbon dioxide gas and liquid water.
Type of reaction:
Balanced Equation using (s, l, g, aq) and Energy:
Spontaneous or Non?
Exo or Endothermic?

5. Liquid dicarbon dihydride reacts with oxygen gas to form carbon dioxide gas and liquid water.
Combustion
2 C2H2 (l) + 5 O2 (g) + energy  4 CO2 (g) + 2 H2O (l) + ENERGY
Nonspontaneous
Exothermic

6. Nitrogen gas reacts with hydrogen gas to produce nitrogen trihydride gas.
Type of reaction:
Balanced Equation using (s, l, g, aq) and Energy:
Spontaneous or Non?
Exo or Endothermic?

7. Nitrogen gas reacts with hydrogen gas to produce nitrogen trihydride gas.
Synthesis (Combination
N2 (g) + 3 H2 (g)  2 NH3 (g) + Energy
Spontaneous
Exothermic

8. Solid aluminum reacts with aqueous iron (II) oxide to make aqueous aluminum oxide and solid iron.
Type of reaction:
Balanced Equation using (s, l, g, aq) and Energy:
Spontaneous or Non?
Exo or Endothermic?

9. Solid aluminum reacts with aqueous iron (II) oxide to make aqueous aluminum oxide and solid iron.
Single Replacement
2 Al (s) + 3 FeO (aq)  Al2O3 (aq) +
3 Fe (s) + Energy
Spontaneous
Exothermic

10. Aqueous aluminum sulfate reacts with aqueous calcium hydroxide to form aqueous aluminum hydroxide and solid calcium sulfate.
Type of reaction:
Balanced Equation using (s, l, g, aq) and Energy:
Spontaneous or Non?
Exo or Endothermic?

11. Aqueous aluminum sulfate reacts with aqueous calcium hydroxide to form aqueous aluminum hydroxide and solid calcium sulfate.
Double Replacement
Al2(SO4)3 (aq) + 3 Ca(OH)2 (aq) 
2 Al(OH)3 (aq) + 3 CaSO4 (s) + Energy
Spontaneous
Exothermic

12. Aluminum + Oxygen gas  ________
Type of reaction:
Names of predicted products:
Balanced Equation:

13. Aluminum + Oxygen gas  ________
Synthesis (Combination) and Combustion
Aluminum oxide
4 Al + 3 O2 + energy  2 Al2O3 + ENERGY

14. Carbon + Water  ________
Type of reaction:
Names of predicted products:
Balanced Equation:

15. Carbon + Water  ________
Single Replacement
Carbon monoxide + Hydrogen gas
C + H2O  CO + H2 + Energy

16. Lithium chlorate  ________
Type of reaction:
Names of predicted products:
Balanced Equation:

17. Lithium chlorate  ________
Decomposition
Lithium chloride + Oxygen gas
2 LiClO3 + Energy  2 LiCl + 3 O2

18. Iron (III) chloride + Ammonium hydroxide  ________
Type of reaction:
Names of predicted products:
Balanced Equation:

19. Iron (III) chloride + Ammonium hydroxide  ________
Double Replacement
Ammonium chloride + Iron (III) hydroxide
FeCl3 + 3 NH4OH  3 NH4Cl + Fe(OH)3 + Energy

20. Tricarbon octahydride + oxygen  ________
Type of reaction:
Names of predicted products:
Balanced Equation:

21. Tricarbon octahydride + oxygen  ________
Combustion
Carbon dioxide + water
C3H8 + 5 O2  3 CO2 + 4 H2O + Energy

22. Aluminum + hydrochloric acid  ________
Type of reaction:
Names of predicted products:
Balanced Equation:

23. Aluminum + hydrochloric acid  ________
Single Replacement
Aluminum chloride + hydrogen gas
2 Al + 6 HCl  2 AlCl3 + 3 H2 + Energy

24. Magnesium + Nitrogen  ________
Type of reaction:
Names of predicted products:
Balanced Equation:

25. Magnesium + Nitrogen  ________
Synthesis (Combination)
Magnesium nitride
3 Mg + N2  Mg3N2 + Energy

26. Barium chloride + aluminum sulfate  ________
Type of reaction:
Names of predicted products:
Balanced Equation:

27. Barium chloride + aluminum sulfate  ________
Double Replacement
Aluminum chloride + Barium sulfate
3 BaCl2 + Al2(SO4)3  2 AlCl3 +
3 BaSO4 + Energy

28. Potassium chlorate  ________
Type of reaction:
Names of predicted products:
Balanced Equation:

29. Sodium carbonate  ________
Decomposition
Sodium oxide + Carbon dioxide
Na2CO3 + Energy  Na2O + CO2