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Rate Law Equation

  • Thread starter TheExibo
  • Start date
55
1
1. The problem statement, all variables and given/known data

Concentration of Hydrochloric Acid (mol/L)

3

2

1.5

1

0.5

Reaction Rate (s/M)

1.333

13.30

38.67

73.00

1466

2. Relevant equations

r=k[H+]m (r is rate in M/s, k is constant, [ ] is concentration, m is order of reaction)

3. The attempt at a solution

I'm not entirely sure how to start off this problem. Using the concentration as the "x" value and the rate of reaction as the "y" value, I need to figure out m, the exponent, and if possible: k, which is the constant. How do I start?
 

Borek

Mentor
27,963
2,470
Can you think of a mathematical way of converting the r=k[H+]m equation to the y=mx+a form (where m is the exponent you are looking for, and all other things - x, y, a - are easy to calculate from the given data?
 
55
1
Can you think of a mathematical way of converting the r=k[H+]m equation to the y=mx+a form (where m is the exponent you are looking for, and all other things - x, y, a - are easy to calculate from the given data?
I am trying that right now. Here is where I've gotten so far:

*using line of best fit slope of the recordings (0.024s-1/M)
log(1/r)=(0.024s-1/M)[H+]+logk
*using random value in the recordings
log0.065=(0.024s-1/M)log3M+logk
-1.19854=logk
k=0.063

I'm also not sure how to get the units for k.
 
18,848
3,654
What would you expect to get if you plotted log(r) vs log(H+)?

Chet
 

epenguin

Homework Helper
Gold Member
3,433
525
To stop this being a very scholastic excercise please show the plot of your fit. We have no idea how good it is nor whether there are any systematic trends away from your line.
Also no one would be treating data of a reaction that he didn't know what it was, and what ws in the reaction mixture, so please tell us.
Does s/M mean the numbers in the second table are reciprocals of the reaction rate?
What does Log3M mean?
 
44
3
Is there any way you could manipulate the given rate to fit the rate law?
 

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