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.
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
NO + ½Cl2 → NOCl
The following initial rates of reaction have been measured experimentally for the given reagent concentrations.
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
