Consider the following data concerning the equation:      H2O2 + 3I– + 2H+ → I3– + 2H2O   [H2O2]   [I–] [H+] rate I 0.100 M   5.00 × 10–4 M 1.00 × 10–2 M 0.137 M/sec II. 0.100 M   1.00 × 10–3 M 1.00 × 10–2 M 0.268 M/sec III. 0.200 M   1.00 × 10–3 M 1.00 × 10–2 M 0.542 M/sec IV. 0.400 M   1.00 × 10–3 M 2.00 × 10–2 M 1.084 M/sec The rate law for this reaction is   a. rate = k[H2O2]2[I–]2[H+]2 b. rate = k[I–] c. None of these d. rate = k[I–][H+] e. rate = k[H2O2][I–][H+] f. rate = k[H2O2][H+]

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Chapter1: Chemical Foundations
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Consider the following data concerning the equation:

     H2O2 + 3I + 2H+ → I3 + 2H2O

 

[H2O2]

 

[I]

[H+]

rate

I

0.100 M

 

5.00 × 10–4 M

1.00 × 10–2 M

0.137 M/sec

II.

0.100 M

 

1.00 × 10–3 M

1.00 × 10–2 M

0.268 M/sec

III.

0.200 M

 

1.00 × 10–3 M

1.00 × 10–2 M

0.542 M/sec

IV.

0.400 M

 

1.00 × 10–3 M

2.00 × 10–2 M

1.084 M/sec


The rate law for this reaction is
 
a. rate = k[H2O2]2[I–]2[H+]2
b. rate = k[I–]
c. None of these
d. rate = k[I–][H+]
e. rate = k[H2O2][I–][H+]
f. rate = k[H2O2][H+]
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