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what is the oxidation number of cl in ocl- ion?

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Lulama Klaas
Lulama KlaasLv10
13 Nov 2020
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Related questions

Balance the following oxidation-reduction reactions that occur inbasic solution. (Use the lowest possible coefficients. Includestates-of-matter under the given conditions in your answer.)

Cl2(g) ? Cl ?(aq) + OCl ?(aq)

I-(aq) + OCl-(aq) IO-(aq) + Cl-(aq)
The above reaction was studied (at a particular temperature) andthe following data were obtained:

[I-]0 [OCl-]0 Initial Rate
(mol/L) (mol/L) (mol L-1 s-1)
0.120 0.160 6.30ƃĀ—10-2
0.030 0.080 7.87ƃĀ—10-3
0.240 0.080 6.30ƃĀ—10-2
0.060 0.160 3.15ƃĀ—10-2

Which of the following expressions for the rate law are completelyconsistent with the above experimental data.

d[Cl-]/dt = k[OCl-]
k[OCl-][I-] = -d[I-]/dt
-d[I-]/dt = k[I-]2[OCl-]
-d[OCl-]/dt = k[I-][OCl-]2
k[OCl-][I-] = d[Cl-]/dt

(Answer with yes/no)

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I have calculated the following values
K = 3.28 L mol^-1 s^-1
k[I^-]^m[OCl^-]^n where m = 1 and n = 1

Not too sure where to go from here. Any help is much appreciated.Thanks! :)

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OClā€“ + Iā€“ OIā€“ + Clā€“ . This rapid reaction gives the following rate data:

(a) Write the rate law for this reaction. (b) Calculate the rate constant with proper units. (c) Calculate the rate when [OClā€“] = 2.0 Ɨ 10-3 M and [Iā€“] = 5.0 Ɨ 10ā€“4 M.

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