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Question

Question #1

At a certain temperature, the equilibrium constant K_c is 0.154 for the reaction 

 

2SO₂ (g) + O₂ (g) <--> 2SO₃ (g)

 

What concentration of SO₃ would be in equilibrium with 0.250 moles of SO₂ and 0.752 moles of O₂  in a 1.00 liter container at this temperature? (note: these latter moles are the equilibrium values. 

 

 

Question #2

 

A+2B <--> C

consider the data

            initial             initial              initial 

             (A)                 (B)                rate

              M                   M                M/min

1          0.23              0.23            0.0048668

2          0.23              0.46            0.0194672

3          0.46              0.46            0.0389344

 

 

If the initial concentrations of both A and B are 0.41M, at what initial rate is C formed?

answer in units of M/min

 

 

 

 

 

 

 

 

Answer 1

For Question 1:

 

The equilibrium constant for the reaction is Kc.  It can be represented as follows:

 

Kc = [SO3]²/([SO2]²[O2])

 

You know the molar concentration of SO2 and O2 to be 0.25M and 0.752M, respectively.  You also know that Kc is 0.154, so you can now solve for the molar concentration of SO3 at equilibrium.  

 

0.154 = [SO3]²/([0.25]²[0.752])

[SO3] = 1.81M

 

For Question 2:

 

You can see from the reaction given that there are twice as many moles of B as there are of A.  This means that the molar concentration of B should be twice that of A.  Therefore, Line 2 is representative data for the reaction given since 0.46M of B is two times 0.23M of A.  The initial rate formation rate of C is 0.0194672 M/min.