I need to find the rate law of a reaction but ive only done so when factors cancel out, this one has all different numbers and im not quite sure what to do with it.
It has time taken every second (which im assuming are the different trials) and different concentrations of OH- .. also under the two concentrations they have data for Abs and ln(abs).. which again i am assuming is absolute value and the ln of absolute value but i don't know how to use this information to find the rate law. Ive only ever solved when it has Trails, data for [1], for [2], and the r initial (M/sec)
To find the rate law of a reaction using the given data, you will need to analyze the relationship between the concentration of OH- and the rate of the reaction. In this case, you have measurements of time, different concentrations of OH-, and corresponding data for Abs (absorbance) and ln(Abs).
Here's a step-by-step guide on how to determine the rate law:
1. Plot the data: Start by plotting the Abs (y-axis) against time (x-axis) for each concentration of OH-. If there is a clear trend in the data, you may be able to infer the order of the reaction by looking at the slope of the plot.
2. Determine reaction order using Abs data: If the Abs values increase or decrease linearly with time, it suggests a first-order reaction. If the Abs values double or quadruple over time, it suggests a second-order (or pseudo-second-order) reaction. Alternatively, you can use the Abs values to calculate the rate constant, k, and compare the values at different concentrations.
3. Determine reaction order using ln(Abs) data: Plot ln(Abs) against time and observe the trend. If the ln(Abs) values decrease linearly with time, it suggests a first-order reaction. If the ln(Abs) values remain constant or decrease exponentially over time, it suggests a zero-order or second-order reaction. Again, you can compare the rate constants from different concentration data.
4. Compare the results: If the reaction order determined from Abs and ln(Abs) data is the same, you can conclude that the reaction follows that particular order. If the results differ, more analysis may be required, considering factors such as reaction mechanism or potential intermediate species.
It's worth noting that the rate law may not always be as straightforward as canceling out factors. In some cases, you may need to use more advanced mathematical techniques, such as integrated rate laws or differential equations, to determine the order and rate constant accurately.
Remember, these are general steps to guide you through the process of determining the rate law. The actual methodology might vary depending on the specific experimental setup and data collected.