reaction like
A+B+C--->D+E+F
If I change only the concentration of C (five different concentrations) keeping concentration of A and B constant, the plot of {concentration of A vs time} will give different initial rates. My detection system will allow me to detect A only at different time.
Now from conc. vs time curve, I can get rate of reaction and as well as concentration of A at different times.
The plot of log rate against log conc. will show up a straight line. The slope will give us the order with respect to reactant C and the intercept will give us the value of rate constant.
The above statement is true or not???
Now since rate constant and orders are constant for a reaction, these two values must be constant at different concentration of reactant C.
In my experiments I found these two values changes at different concentrations of starting materials. Also the plot of log rate vs log concentration becomes nonlinear (curve).
What could be the reason for this???
I need your help.
For example
[A] [C] Temp. Initial rate rate constant Order
0.1 0.1 0.1 25 2.27E-04 0.238 3.01823
0.1 0.2 0.1 25 5.94E-04 660.29 6.0387
0.1 0.3 0.1 25 7.82E-04 9.88E-04 0.10158
0.1 0.4 0.1 25 1.49E-03 0.0628 1.6162
0.1 0.5 0.1 25 4.52E-03 61.31 3.98585