Question

In a 500 ml capacity vessel CO & CL2 are mixed to form cocl2. at equilibrium, it contains 0.2moles of cocl2& 0.1mole of each of co & cl2. the equilibrium constant for the reaction co+cl2=cocl2 is ????

Answer 1

Answer in the pic above.

Answer 2

Answer : The equilibrium constant for the given reaction is 10 L/mole.

Solution : Given,

Volume = 500 ml = 0.5 L                         (1 L = 1000 ml)

The balanced chemical equilibrium reaction is,

                                     $CO(g)+Cl_2(g)\rightleftharpoons COCl_2(g)$

At equilibrium (moles)        0.1        0.1            0.2

First we have to calculate the concentration of each gas molecules.

Formula used :     $Concentration=\frac{Moles}{Volume(L)}$

Concentration of CO gas = $\frac{0.1}{0.5}=0.2mole/L$

Concentration of $Cl_2$ gas = $\frac{0.1}{0.5}=0.2mole/L$

Concentration of $COCl_2$ gas = $\frac{0.2}{0.5}=0.4mole/L$

The expression for equilibrium constant for reaction is,

$K_c=\frac{[COCl_2]}{[CO][Cl_2]}$

Now put all the given values in this expression, we get the value for equilibrium constant.

$K_c=\frac{(0.4mole/L)}{(0.2mole/L)(0.2mole/L)}=10L/mole$

Therefore, the equilibrium constant for the given reaction is 10 L/mole.