Calculate kinetic orders using three measured experiments. See constants, predictions, and graph outputs instantly. Learn reaction trends with guided chemistry steps.
Enter three experimental trials. The calculator solves the reactant orders and the total order from the measured rate data.
The chart compares measured rates, predicted rates, and calculated orders.
| Experiment | [A] | [B] | Rate | Interpretation |
|---|---|---|---|---|
| 1 | 0.10 | 0.10 | 0.020 | Baseline trial |
| 2 | 0.20 | 0.10 | 0.080 | Doubling A quadruples rate |
| 3 | 0.20 | 0.20 | 0.160 | Doubling B doubles rate |
The overall reaction order equals the sum of all partial orders. For two reactants, total order = x + y.
Using experiment ratios removes k. The calculator solves these logarithmic equations:
After solving x and y, the tool estimates k from each experiment and reports the average value.
Overall reaction order is the sum of the exponents in the rate law. It describes how the total reaction rate changes when all reactant concentrations change.
Three experiments provide enough information to solve for two unknown reactant orders and then verify the fit using a third data point and predicted rates.
No. Concentrations and rates must be positive because the method uses logarithms. Zero or negative values make the logarithmic equations undefined.
A fractional order shows that the rate does not change by a simple whole-number pattern. It often appears in complex mechanisms or multistep reactions.
If the experiments do not vary concentrations independently, the equations become dependent. Then the determinant becomes zero and unique orders cannot be found.
The rate constant scales the entire rate law. After the orders are found, k is computed from each experiment and averaged for a representative value.
Predicted rates help you compare the fitted rate law with measured data. Small errors suggest the experimental model matches the entered kinetics well.
Yes. Use any consistent concentration and rate units. The computed orders remain unchanged, though the numerical value and units of k may differ.
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