Calculating Equilibrium Constants Worksheet 3:  Additional equilibrium constant problems

 

1.        (a) Write the equilibrium constant expression for this reaction:  N2 (g)  + O2 (g) 2 NO  (g).

(b) At 2130oC the equilibrium constant for this reaction is 0.0025.  If [N2] =0.81 M, [O2] = 0.75 M and [NO] = 0.030 M, calculate the value of the reaction quotient Q and determine the direction the reaction will proceed to achieve equilibrium

 

 

 

 

 

 

 

 

2.         (a) Write the equilibrium constant expression for this reaction:  CO (g)  + H2O (g) H2 (g) + CO2 (g)

(b) At 527oC the equilibrium constant for this reaction is 5.10.  If [CO] =0.15 M, [H2] = 0.25 M, [H2O] = 0.42 M and  [CO2] = 0.37 M, calculate the value of the reaction quotient Q and determine the direction the reaction will proceed to achieve equilibrium

 

 

 

 

 

 

 

 

3.         (a) Write the equilibrium constant expression for this reaction:  SbCl5 (g) SbCl3  (g)    +  Cl2 (g).

(b) At 448oC the equilibrium constant for this reaction is 0.0251.  If [SbCl5] =0.095 M, [SbCl3] = 0.020 M and [Cl2]  = 0.050 M, calculate the value of the reaction quotient Q and determine the direction the reaction will proceed to achieve equilibrium

 

 

 

 

 

 

 

 

 

4.         (a) Write the equilibrium constant expression for this reaction:  2 HF  (g). H2 (g)  + F2 (g)

(b) At 1000oC the equilibrium constant for this reaction is 1.0 x 10-13.  If [HF] =23.0 M, [H2] = 0.540 M and [F2] = 0.380 M, calculate the value of the reaction quotient Q and determine the direction the reaction will proceed to achieve equilibrium

 

 

 

 

 

 

 

 

5.        (a) Write the equilibrium constant expression for this reaction:  2 SO2  (g)  + O2 (g) 2 SO3  (g) 

(b) At 1227oC the equilibrium constant for this reaction is 0.15.  If [SO2] =0.344 M, [O2] = 0.172 M and [SO3] = 0.056 M, calculate the value of the reaction quotient Q and determine the direction the reaction will proceed to achieve equilibrium