2HgCl2(aq) + C2O42–(aq) 2Cl–(aq) +2CO2(g) + Hg2Cl2(s) The above reaction was stu

Question

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

[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

Explanation / Answer

answer : first-order wrt HgCl2, second-order wrt C2O42–, third-order overall , k = 7.6x10–3 M–2min–1    

explanation :

rate= k [HgCl2]x [C2O4-2]y

data1 ,2,3

1.8x 10-5=k [0.105]x [0.15]y ------------->(1)

7.2x 10-5=k [0.105]x [0.30]y ------------------> (2)

3.6x 10-5=k [0.0525]x [0.30]y ------------------> (3)

by solving 1 and 2 we get y= 2

by solving 2 and 3 we get x =1

rate= k [HgCl2]1 [C2O4-2]2

total order = 1+2 = 3

from 1

1.8x 10-5=k [0.105]1 [0.15]2 ------------->(1)

k = 7.6 x 10^-3 M–2min–1   

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