Equilibrium Calculations

 

   1) The following reaction has an equilibrium constant of 0.083 at 900°C.

COCl2(g) CO(g) + Cl2(g)

If you have 1.00 mole of COCl2(g) in a 1.00-L container initially, how many moles of COCl2 will be present when the system reaches equilibrium?

(a) 0.75 moles

(b) 0.89 moles

(c) 0.71 moles

(d) 0.96 moles

 

   2) You have 0.50 mol SbCl5 present initially in a 1.0-L flask. The system is allowed to reach equilibrium at 450ºC as shown below.

SbCl5(g) SbCl3(g) + Cl2(g)

There is 0.10 mol Cl2 present at equilibrium. What is K?

(a) 2.0 x 10-2

(b) 2.5 x 10-2

(c) 1.0 x 10-1

(d) 4.0 x 101

(e) 5.0 x 101

 

   3) The following reaction has an equilibrium constant of 0.050 at a given temperature.

N2(g) + O2(g) 2NO(g)     

If you have 0.75 moles of N2(g) and 0.75 moles of O2(g) in a 2.0-L container initially, how many moles of N2 will be present when the system reaches equilibrium?

(a) 0.67 moles

(b) 0.73 moles

(c) 0.61 moles

(d) 0.74 moles

(e) 0.34 moles

 

   4) You have 0.80 moles NH3 and 0.80 moles O2 present initially in a 4-L flask. You allow the reaction to run until it reaches equilibrium as shown below.

2NH3(g) + 2O2(g) 2N2O(g) + 3H2O(g)

Which of the following is the correct ICE table for this equilibrium?

(a)

NH3
O2
N2O
H2O
[]i 
 0.8
 0.8
  0
   0
[]c
-2x
-2x
+x
+3x
[]e
0.8 - 2x
0.8 - 2x
  x
  3x

(b)

NH3
O2
N2O
H2O
[]i 
 0.2
 0.2
   0
   0
[]c
-6x
-6x
+6x
+6x
[]e
0.2 - 6x
0.2 - 6x
  4x
  4x

(c)

NH3
O2
N2O
H2O
[]i 
 0.8
 0.8
  0
  0
[]c
-x
-x
+x
+x
[]e
0.8 - x
0.8 - x
  x
  x

(d)

NH3
O2
N2O
H2O
[]i 
 0.2
 0.2
  0
  0
[]c
-2x
-2x
+x
        +3x
[]e
0.2 - 2x
0.2 - 2x
  x
 3x

 

   5) You have 0.80 moles NH3 and 0.40 moles O2 present initially in a 4-L flask. You allow the reaction to run until it reaches equilibrium as shown below.

4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)

Which of the following is the correct ICE table for this equilibrium?

 

(a)

NH3
O2
N2O
H2O
[]i 
 0.80
 0.40
  0
  0
[]c
  -x
-x
+x
+x
[]e
0.80 - x
0.40 - x
  x
  x

(b)

NH3
O2
N2O
H2O
[]i 
 0.20
 0.10
   0
   0
[]c
-4x
-5x
+4x
+6x
[]e
0.20 - 4x
0.10 - 5x
  4x
  6x

(c)
NH3
O2
N2O
H2O
[]i 
 0.80
 0.40
   0
   0
[]c
-4x
-5x
+4x
+6x
[]e
0.20 - 4x
0.40 - 5x
  4x
  6x

(d)

NH3
O2
N2O
H2O
[]i 
 0.20
 0.10
     0
     0
[]c
-30x
-30x
+30x
        +30x
[]e
0.20 - 30x
0.10 - 30x
  30x
 30x

 

   6) The following reaction has an equilibrium constant of 50. at a given temperature.

I2(g) + H2(g) 2HI(g)     

If you have 0.59 moles of I2(g) and 0.59 moles of H2(g) in a 0.50-L container initially, how many moles of H2 will be present when the system reaches equilibrium?

(a) 0.14 moles

(b) 0.02 moles

(c) 0.13 moles

(d) 0.070 moles

(e) 0.26 moles

 

   7) You have 0.50 mol each of H2O and Cl2O present initially in a 1.0-L flask. The system is allowed to reach equilibrium at 25ºC as shown below.

H2O(g) + Cl2O(g) 2HOCl(g)

There is 0.13 mol HOCl present at equilibrium. What is K?

(a) 8.9 x 10-2

(b) 6.8 x 10-2

(c) 6.8 x 10-1

(d) 1.2 x 10-1

(e) 1.0

 

    8) The following reaction has an equilibrium constant, Kc, of 12 at 900°C.

CO(g) + Cl2(g) COCl2(g)

If you have 0.57 moles of Cl2(g) and 0.57 moles of CO(g) in a 1.0-L container initially, how many moles of CO will be present when the system reaches equilibrium?

(a) 0.020 moles

(b) 0.18 moles

(c) 0.040 moles

(d) 0.50 moles

 

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