# Chemistry Question helpy

**URL:** <https://forum.kirupa.com/t/chemistry-question-helpy/222403>\
**Category:** random\
**Created:** [April 13, 2007, 2:06am UTC](https://forum.kirupa.com/t/chemistry-question-helpy/222403 "2007-04-13T02:06:41Z")\
**Posts on this page:** 1\
**Page:** 1

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**Author:** ![cptn\_nemo](https://avatars.discourse-cdn.com/v4/letter/c/8edcca/32.png) [@cptn\_nemo](https://forum.kirupa.com/u/cptn_nemo)\
**Post date:** [April 13, 2007, 2:06am UTC](https://forum.kirupa.com/t/chemistry-question-helpy/222403/1 "2007-04-13T02:06:41Z")

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Hi ever1!

We recently conducted a rate law lab in class to determine the order of a simple reaction. It was measureing the time required for Mg strip to react w/ HCl solutions in various concentration (4.0mol/L, 3.0, 2.0, 1.0)  
Mg(s) + 2H^+ (aq) --\> H2 (g) + Mg^2+ (aq) the Cl^- ion is a spectator only

It says:

- "General rate law expression for this reaction is: rate=k[H+]^n where n is the order of the reaction. The rate can be expressed in terms of reciprocal time since the concentration of the Mg is constant. So, rate = 1/t and 1/t=k[H+]^n. Then take the natural logs of both sides,  
giving: ln(1/t) = n ln[H+] + ln k  
which now has the form of a linear equation, where n is the order of reaction and k is rate constant.\*

I have managed to plot the graph on ln(1/t) vs ln[H+], finding the slope, y intercept and r^2. So problem is that i do not understand how to find the order of reaction relative to the [H+] and the rate law constant. Plz help

R^2 = 0.968  
Y-intercept = -3.798  
Slope = 1.439