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    Gernald Posts: 901, Reputation: 93
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    Feb 17, 2009, 03:28 PM
    Kinetics: rate equations
    I'm working on a lab and am going to ask my proff. About this tomorrow but was wondering if anyone could help me out with this.

    I need to find the rate equation for a reaction: So far I have the following:

    Reaction Number Log Initial [NH4^1+] Log Initial [NO2^1-] Log Rate of Reaction
    1 -2.00E+00 -6.99E-01 -6.27E+00
    2 -1.70E+00 -6.99E-01 -5.97E+00
    3 -1.40E+00 -6.99E-01 -5.67E+00
    4 -1.22E+00 -6.99E-01 -5.49E+00
    5 -6.99E-01 -1.69E+00 -5.97E+00
    6 -6.99E-01 -1.39E+00 -5.67E+00
    7 -6.99E-01 -1.22E+00 -5.49E+00
    8 -6.99E-01 -1.09E+00 -5.36E+00

    I know that for 1-4:
    Equation of Treadline: y = 0.9976x - 4.2722
    Slope of Treadline (a): 0.997594478
    Intercept (logK'app): 4.272245664

    And 5-8:
    Equation of Treadline: y = 1.0013x - 4.27
    Slope of Treadline (b): 1.001262009
    Intercept (logK'app): -4.269973374

    Now I need to find the constant K and am so confused... how do I do it? Do I plug it in to
    K'app=K[NO2]^a or something else, I'm also confused I think because won't the rate change if rate=K'app[NH4]^a?? And will I get two different K's for each NO2 and NH4 ?

    Thanks for any help, I just want to understand it and what I'm supposed to do.

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