The equilibrium constant, Kc, for the following
reaction is 55.6 at 698 K:
H2(g) +
I2(g)
---------->2HI(g)
1) Calculate the equilibrium concentrations of reactants and
product when 0.309 moles of
H2 and 0.309 moles of
I2 are introduced into a 1.00 L vessel
at 698 K.
| [H2] | = | M? |
| [I2] | = | M? |
| [HI] | = | M? |
2.The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K:
An equilibrium mixture of the three gases in a 1.00 L flask at
500 K contains 0.210 M
PCl5,
5.02×10-2 M
PCl3 and
5.02×10-2 M
Cl2. What will be the concentrations of
the three gases once equilibrium has been reestablished, if
4.12×10-2 mol of
PCl3(g) is added to the
flask?
| [PCl5] | = | M? |
| [PCl3] | = | M? |
| [Cl2] | = | M? |
3.The equilibrium constant, K, for the following reaction is 5.01×10-2 at 538 K:
An equilibrium mixture of the three gases in a
16.4 L container at 538 K
contains 0.153 M PCl5,
8.74×10-2 M
PCl3 and
8.74×10-2 M
Cl2. What will be the concentrations of
the three gases once equilibrium has been reestablished, if the
equilibrium mixture is compressed at constant temperature to a
volume of 7.71 L?
| [PCl5] | = | M? |
| [PCl3] | = | M? |
| [Cl2] | = | M? |
4. The equilibrium constant, Kp, for the following
reaction is 55.6 at 698 K:
H2(g) +
I2(g)
----------->2HI(g)
If ΔH for this reaction is -10.4 kJ, what is the
value of Kp at 623 K?
Kp = ?
1) H2(g) + I2(g) ----------> 2HI(g)
initial 0.309 M 0.309 M -
change -x -x +2x
equil 0.309-x 0.309-x 2x
Kc = [HI]^2/[H2][I2]
55.6 = (2X)^2/(0.309-X)^2
at equilibrium,
[HI] = 2X = 2*0.244 = 0.488 M
[I2] = 0.309-0.244 = 0.065 M
[H2] = 0.309-0.244 = 0.065 M
2)
PCl5(g)-------> PCl3(g) + Cl2(g)
equil 0.21
M
0.0502 M 0.0502 M
added - 0.0412 M -
change +x -x -x
equil 0.21+x 0.0914-x 0.0502-x
Kc = [PCl3][Cl2]/[PCl5]
1.2*10^-2 = (0.0914-x)(0.0502-x)/(0.21+x)
x = 0.015
at equilibrium,
[PCl3] = 0.0914-0.015 = 0.0764 M
[Cl2] = 0.0502-0.015 = 0.0352 M
[Pcl5] = 0.21+0.015 = 0.225 M
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