# Rate Law Equation

1. Mar 21, 2015

### TheExibo

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?

2. Mar 21, 2015

### Staff: Mentor

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?

3. Mar 21, 2015

### TheExibo

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.

4. Mar 21, 2015

### Staff: Mentor

What would you expect to get if you plotted log(r) vs log(H+)?

Chet

5. Mar 21, 2015

### epenguin

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?

6. Mar 22, 2015

### Teemo

Is there any way you could manipulate the given rate to fit the rate law?