For the following reaction, Kc = 255 at 1000 K. CO(g)+Cl2(g)⇌COCl2(g) A reaction mixture initially contains a CO concentration of 0.1550 M and a Cl2 concentration of 0.172 M at 1000 K.

What is the equilibrium concentration of CO at 1000 K?

What is the equilibrium concentration of Cl2 at 1000 K?

What is the equilibrium concentration of COCl2 at 1000 K?

Given reaction is:

  0.1550  0.172         O initial

0.1550-x   0.172-x      x Equilibrium

Now,

→

By substituting the values, we get

or,

                                      (correct value)

(a)

Equilibrium constant of [CO],

=

=

(b)

Equilibrium constant of [Cl₂],

=

=

(c)

Equilibrium constant of [COCl₂],

=

=

Thus the above responses are correct.

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The equilibrium concentration of CO at 1000 K is 0.016 M , the equilibrium concentration of at 1000 K is= 0.033 M  and the equilibrium concentration of at 1000 K is 0.139 M  

Explanation:

Initial concentration of  

Initial concentration of  

The given balanced equilibrium reaction is,

Initial conc.           0.1550 M           0.172 M          0 M

At eqm. conc.    (0.1550-x) M      (0.172-x) M     (x) M

The expression for equilibrium constant for this reaction will be,

we are given :

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

Thus the equilibrium concentration of CO at 1000 K is= (0.1550-x) M =(0.1550-0.139) M = 0.016 M  

Thus the equilibrium concentration of at 1000 K is= (0.172-x) M =(0.172-0.139) M = 0.033 M  

Thus the equilibrium concentration of at 1000 K is= x M = 0.139 M  

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml