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aliya0001 [1]
3 years ago
9

Phosphorous pentachloride decomposes according to the reaction

Chemistry
1 answer:
guajiro [1.7K]3 years ago
4 0

Answer: The equilibrium constant, K_c, for the reaction is 0.061.

Explanation:

Initial concentration of PCl_5  = \frac{\text {given mass}}{\text {Molar mass}\times Volume in L}}=\frac{12.3g}{208.2g/mol\times 1.50L}=0.039M  

Equilibrium concentration of PCl_5 = \frac{31.8}{100}\times 0.039=0.012M  

The given balanced equilibrium reaction is,

                            PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)

Initial conc.              0.039 M                0 M        0 M

At eqm. conc.     (0.039-x) M              (x) M   (x) M

Given : (0.039-x) = 0.012

x = 0.027

The expression for equilibrium constant for this reaction will be,

K_c=\frac{[Cl_2]\times [PCl_3]}{[PCl_5]}

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

K_c=\frac{0.027\times 0.027}{0.012}=0.061

The equilibrium constant, K_c, for the reaction is 0.061.

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