\

Step 1: \ \

\
\
\

The chemical equation is \"\".

\

Initial concentration of Br2 is 0.063 M.

\

Initial concentration of Br is 0.012 M.

\

Equilibrium constant of the reaction is \"\". \ \

\

1 mole of Br2 decomposes to 2 moles of Br.

\

Let \"\" be the change in concentration of Br2 ,

\

then change in concentration of Br be \"\".   (negative sign indicates decomposition)

\

Step 2:

\

Construct an ICE table.

\

Equilibrium Amount = Initial amount + Change in amount.

\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \
                                        \"\"
Initial Amount\"\"\"\"
Change in Amount\"\"\"\"
Equilibrium amount\"\"\"\"
\

Find the equilibrium constant of the reaction.

\

The chemical equation is \"\".

\

Equilibrium constant \"\".

\

\"\".

\

But equilibrium constant given as \"\". \ \

\

\"\"

\

Step 3:

\

Now solve for x .

\

\"\"

\

Find the equilibrium amount of Br2 : \"\".

\

\"\"

\

Find the equilibrium amount of Br : \"\" .

\

\"\"

\

So the equilibrium amount of Br is 0.00844 M. \ \

\

The equilibrium amount of Br2 is 0.06478 M.

\

Solution:

\

The equilibrium amount of Br is 0.00844 M. \ \

\

The equilibrium amount of Br2 is 0.06478 M.

\
\
\

 

\
 
\
 
\