# Reaction Energy, Kinetics Problems

1)      For each reaction listed below, determine the ?H and type of reaction (endothermic or exothermic)

a.       2CO(g)  +  2NO(g)  ->  N2(g)  +  CO2(g)  +  746.8kJ

b.      2Al(s)  +  3/2 O2(g)  ->  Al2O3(s)  +  1675.7kJ

c.       2NaHCO3(s)  +  129kJ  ->  Na2CO3(s)  +  H2O(g)  +   CO2(g)

d.      2HCl(g)   +  184.6kJ  ->  H2(g)  +  Cl2(g)

e.       N2H4(g)  +  3O2(g)  ->  2NO2(g)  +  2H2O(g)  +  197.8kJ

2)      Rewrite each reaction below with the ?H value in its appropriate position and identify the reaction as endothermic or exothermic.

a.       ½N2(g)  +  O2(g)  ->  NO2(g)

?H = 33.15kJ

b.      Mg(s)  +  Cl2(g)  ->  MgCl2(s)

?H =  –641.2kJ

c.       Si(s)  +  2Cl2(g)  ->  SiCl4(l)

?H =  –687.1kJ

d.      CO2(g)  ->  CO(g)  +  ½O2(g)

?H =  283.0kJ

e.       H2O(g)  +  C(s)  ->  CO(g)  +   H2(g)

?H =  131.3kJ

3)      Increasing temperature increases the rate of a reaction.  What are the other 4 factors affecting reaction rate?  Why does a higher temperature increase reaction rate?

4)      Write equilibrium constant expressions for each reaction in #1 (a-e).  Ignore the ?H value in reactions.  The only thing to remember is whether the compounds are gases / aqueous solutions, or solids / liquids.

a.                                                   d.

b.                                                   e.

c.

5)      Write equilibrium constant expressions for each reaction in #2 (a-e).  Ignore the ?H value in reactions.

a.                                                   d.

b.                                                   e.

c.

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