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Chemistry Forums for Students => Physical Chemistry Forum => Topic started by: matsci0000 on January 09, 2010, 11:45:07 AM

Title: Chemical Kinetics
Post by: matsci0000 on January 09, 2010, 11:45:07 AM

The following data are obtained for the initial rates of then reaction for A+2B+C----->2D+E
Experiment..[A]....[C]..Initial rate
1                   1.40     1.40     1.00        R1
2                   0.70     1.40     1.00        R2=(R1)/2
3                   0.70     0.70     1.00       R3=(R2)/4
4                   1.40     1.40      0.50      R4=16R3
5                   0.70      0.70      0.50      R5=?
a)What is the order of the reaction with respect to A,B,C?
b)What is the value of R5 in terms of R1.

Title: My answer
Post by: matsci0000 on January 09, 2010, 11:47:43 AM

Middle row indicates the concentrations of B.

I got the orders 1,2,and -4 respectively.
Can any one just verify?? :-\

Title: Re: Chemical Kinetics
Post by: Schrödinger on January 09, 2010, 11:56:05 AM

Are you sure the data for experiment 4 is correct?

Title: Re: Chemical Kinetics
Post by: matsci0000 on January 09, 2010, 12:39:52 PM

Yes,there was an error in the data of experiment 4 .I've corrected this error.

Title: Re: Chemical Kinetics
Post by: sjb on January 09, 2010, 01:44:11 PM

Can you write the rate of experiment 4 in terms of the rate of experiment 1?

Then you can see what happens when you half each of the rates in turn, and so apply to R5