Calculate the amounts of each substance in the reaction below if an initial amount of 0.400 moles are brought together with an initial amount of 2.29 moles of Cl2 in a 1.00 L vessel

Complete Question

Calculate the equilibrium amounts of each substance in the reaction below if an initial amount of 0.400 moles of CO are brought together with an initial amount of 2.20 moles of Cl2 in a 1.00 L vessel and then equilibrium is established at 900 K. Kc at this temperature = 0.800. COCl2(g)  CO(g) + Cl2(g)

The amount of each substance at equilibrium is  

Explanation:

From the question we are told that  

    The initial amount of CO  is

    The initial amount of   is  

     The volume of the vessel  is  

     The temperature is  

     The equilibrium constant at the given temperature is  

The reaction is  

Now Generating an I C  E table  

Initial [I]                       0                          0.400                 2.20

Change [C ]                + x                           -x                       - x    

Equilibrium [E  ]            x                          0.400- x            2.20 - x

Here  x  is the amount in terms of concentration by which and   and   decreased during the reaction

Generally the equilibrium constant is mathematically represented as  

=>      

=>        

=>          

Generally at equilibrium the amount of   present is

Generally the equilibrium the amount of    present is

=>    

Generally the equilibrium the amount of    present is

=>      

the ratio of the conjugate base to the acid required to attain the desired ph.