Question

2HgCl2(aq) + C2O42–(aq) → 2Cl–(aq) +2CO2(g) + Hg2Cl2(s)

Answer 1

Explanation:

Expression for rate of the given reaction is as follows.

             Rate = k[HgCl_{2}]x [C_{2}O^{2-}_{4}]y[/tex]

Therefore, the reaction equations by putting the given values will be as follows.

       $1.8 \times 10^{-5} = k[0.105]x [0.15]y$ ............. (1)

       $7.2 \times 10^{-5} = k [0.105]x [0.30]y$ ........... (2)

       $3.6 \times 10^{-5} = k [0.0525]x [0.30]y$ ............ (3)

Now, solving equations (1) and (2) we get the value of y = 2. Therefore, by solving equation (2) and (3)  we get the value of x = 1.

Therefore, expression for rate of the reaction is as follows.

     Rate = $k[HgCl_{2}]x [C_{2}O^{2-}_{4}]y$

          Rate = $k [HgCl2]1 [C_{2}O^{-2}_{4}]2$

Hence, total order = 1 + 2 = 3

According to equation (1),

               $1.8 \times 10^{-5} = k[0.105]x [0.15]y$  

            $1.8 \times 10^{-5} = k [0.105]1 [0.15]2$  

                      k = $7.6 \times 10^{-3} M^{-2} min^{-1}$  

Thus, we can conclude that rate constant for the given reaction is $7.6 \times 10^{-3} M^{-2} min^{-1}$.