2hgcl2(aq) + c2o42–(aq) → 2cl–(aq) +2co2(g) + hg2cl2(s)

the above reaction was studied by the method of initial rates and the following results were obtained:

[hgcl2] (m)

[c2o42–] (m)

initial rate (m/min)

0.105

0.15

1.8x10–5

0.105

0.30

7.2x10–5

0.0525

0.30

3.6 x10–5

0.0525

0.15

9.0x10–6

how would you describe the kinetics of this reaction? what is the rate constant?

first-order wrt hgcl2, second-order wrt c2o42–, third-order overall

k = 7.6x10–3 m–2min–1

first-order with respect to (wrt) hgcl2, first-order wrt c2o42–, second-order overall

k = 1.1x10–3 m–1min–1

zero-order wrt hgcl2, second-order wrt c2o42–, second-order overall

k = 5.4x10–5 mmin–1

first-order wrt hgcl2, second-order wrt c2o42–, second-order overall

k = 4.3x10–8 m–2min–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)

        ........... (2)

        ............ (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 =

          Rate =

Hence, total order = 1 + 2 = 3

According to equation (1),

                      k =  

Thus, we can conclude that rate constant for the given reaction is .

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you gotta add the following molecules so we can give u an answer

explanation: