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GalaxieFiable2952

Nitric oxide gas (NO) reacts with chlorine gas according to the chemical equation given below.

NO + ½Cl2 → NOCl

The following initial rates of reaction have been measured experimentally for the given reagent concentrations.

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Which of the following is the rate law (rate equation) for this reaction?

Select one:

A. rate = k[NO]

B. rate = k[NO][Cl2]

C. rate = k[NO]2[Cl2]

D. rate = k[NO]2[Cl2]2

E. rate = k[NO][Cl2]1/2

For NO I did Expt 2/ Expt1 = 4.79/1.19= (1.00/0.50) exponent x

For Cl2 I did expt 3/ expt 2= 9.59/4.79= (1.00/0.50) exponent y

Here I am stuck into how to figure out the exponent value for each

Emilie L

Good afternoon Brit! 

Thank you for your question :).

I am unfortunately unable to access the link you shared. However, I think that you may find a similar exercise as yours by clicking on the following link :

https://www.alloprof.qc.ca/fr/eleves/bv/chimie/la-loi-de-vitesse-de-reaction-c1034

Let us know if you have any other questions or if you need more precision.

Good luck! 

Emilie