[spartanR]

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

[bjraines]

you find the order of the reaction from the graph itself. plot each equation, the one the gives you the straight line is the order of the reaction.

if you mean rate constant k,

you said above that the intercept is ln k

so take tha vaule and put in the exponent of e