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 determine the rate law of a reaction based on the given information, you can use the method of initial rates. Here's how you can approach it:
1. Collect the data for the different trials and their corresponding concentrations of OH-, time taken, Abs (absorbance), and ln(Abs) values.
2. Recognize that the rate law is determined by the relationship between the concentration of the reactants and the reaction rate. The general form of a rate law equation is: Rate = k[A]^m[B]^n[C]^p, where k is the rate constant, and m, n, and p represent the order of reaction with respect to each reactant.
3. To determine the order with respect to OH-, you can analyze the effect of changing its concentration on the rate of the reaction. Look for trials where the concentration of OH- changes while keeping the concentrations of other reactants constant. Compare the rates obtained in these trials and determine if doubling the concentration of OH- doubles the rate, triples the rate, etc. This will give you the order of the reaction with respect to OH-. Note that if changing the concentration of OH- has no effect on the reaction rate, its order is 0.
4. Once you've determined the order with respect to OH-, you can further analyze the relationship between the concentration of OH- and the ln(Abs). If the data shows a linear relationship between ln(Abs) and time, it suggests that the reaction follows a first-order kinetics, i.e., the rate is directly proportional to the concentration of OH-. In this case, the rate law would simply be Rate = k[OH-].
5. However, if the relationship between ln(Abs) and the concentration of OH- is not linear, it suggests a more complex reaction mechanism. In such cases, you may need to perform additional analyses or consult the given experimental conditions to find the appropriate rate law equation.
Note: Abs typically stands for absorbance, which is a measure of the amount of light absorbed by a solution. It is different from the absolute value. In some cases, absorbance is used as an indirect measure of concentration, hence the relationship between Abs and ln(Abs) may provide insights into the reaction kinetics.
Remember, this is a general approach, and the specific method to determine the rate law may vary depending on the experimental setup and data provided.