Chemistry – Equilibrium
Tall: 1)
Name: _______________________Date: _________- Period: _______
The decomposition of CaCO3 is an endothermic process:
CaCO3(s)  CaO(s) + CO2(g)
a) Use LeChatelier’s Principle to explain how an increase in temperature would affect the
equilibrium.
b) If more CaCO3 is added to a flask in which this equilibrium exists, how is the equilibrium
affected?
c) If pressure within a flask in which this equilibrium exists is increases, how is the
equilibrium affected?
2)
Write equilibrium constants for the following reactions:
a)
(NH4)2CO3(s)  2 NH3(g) + CO2(g) + H2O(g)
b)
CO(g) + ½ O2(g)  CO2(g)
d) Fe2+(aq) + Sn(s)  Sn2+(aq) + Fe(s)
e) N2O4(g) + O3(g)  N2O5(g) + O2(g)
3)
Neither PbCl2 nor PbF2 are appreciably soluble in water. If solid PbCl2 and solid PbF2 are
placed in separate beakers, in which beaker is the [Pb2+] greatest? Explain your choice. The
equilibrium constants for the solids dissolving in water are:
PbCl2(s)  Pb2+(aq) + 2 Cl¯(aq)
PbF2(s)  Pb2+(aq) + 2 F¯ (aq)
K = 1.7x10-5
K = 3.7x10-8
Chemistry – Equilibrium
Name: _______________________Date: _________- Period: _______
Grande
4)
The reaction below has an equilibrium constant, Keq, of 171 at 25oC. Using the reaction
conditions given, determine if the reaction is product-favored, reactant-favored, or at
equilibrium. Don’t forget to find Molarity first!
2 NO2(g)  N2O4(g)
a) 2.0x10-3 mol NO2, 1.5x10-5 mol N2O4, 10.0 L flask
b) 1.5x10-4 mol NO2, 2.0x10-3 mol N2O4, 10.0 L flask
c) 2.0x10-3 mol NO2, 1.5x10-3 mol N2O4, 5.0 L flask
5)
At room temperature the equilibrium constant Keq for the reaction:
2NO(g)  N2(g) + O2(g)
is 1.4x1030. In the atmosphere at room temperature the concentration of nitrogen gas is 0.33
mol/L and the concentration of oxygen gas is about 25% that value. Calculate the equilibrium
concentration of nitrogen monoxide in the atmosphere.
Venti
6)
A 1.00 mol sample of CO2 is heated to 1000K with excess graphite in a container of volume
40.0 L. At this temperature, Kc is 2.11x10-2 for the reaction:
C(graphite) + CO2(g)  2 CO(g)
a)
b)
What are the equilibrium concentrations of each species?
If the volume of the flask is changed so a new equilibrium is established in which the
amount of CO2 in the flask equals the amount of CO, what is the new volume of the flask?