If 0.64 mol PCl5 is placed in a 1.0 L flask and allowed to reach equilibrium at a given temperature, what is the final concentration of Cl2 in the flask? PCl5 (g)→ PCl3 (aq) + Cl2 (g) Kc= 0.47

The final concentration of at equilibrium is 0.36 M

Explanation:

Moles of   = 0.64 mole  

Volume of solution = 1.0 L

Initial concentration of =

The given balanced equilibrium reaction is,

Initial conc.       0.64 M         0M        0M  

At eqm. conc.     (0.64-x) M   (x) M      (x) M

The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get

By solving the term 'x', we get :

x = 0.36

Thus, the final concentration of at equilibrium is x = 0.36 M

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