Qs about chemical kinetic 1) why is the general rate law transformed to a natura
ID: 691257 • Letter: Q
Question
Qs about chemical kinetic 1) why is the general rate law transformed to a naturallogarithmic form during the calculations of the rate law in thisexperiment? 2) what experimental factors change the numerical value of nin the rate law for thr reaction of H2O2 with I? Assume that thetemperature in constant. 3)what experimental factors change the numerical value of k inthe rate law for the reaction of H202 with I? Qs about chemical kinetic 1) why is the general rate law transformed to a naturallogarithmic form during the calculations of the rate law in thisexperiment? 2) what experimental factors change the numerical value of nin the rate law for thr reaction of H2O2 with I? Assume that thetemperature in constant. 3)what experimental factors change the numerical value of k inthe rate law for the reaction of H202 with I?Explanation / Answer
This is actually more of a mathematics question, but I will attempt to explain it here anyway. It will involve some knowledge of calculus however. The equation for general rate law for a first order reaction is given as follows: r = -(d/dt)[A] = k[A] This means that the rate of the reaction is dependent only on one of the reactants. Integrating this equation allows us obtain the slope of the reaction from plotted data since a graph of ln[A] vs time gives a straight line with a slope of -k. When you integrate both sides of the equation -(d/dt)[A] = k[A], you'll notice the natural logs appear: Rearrange d[A]/[A] = - k dt Integrate with defined limits: ? d[A]/[A] = -k ? dt where [A] limits are defined from [A]o --> [A] and t limits are defined from t0 --> t ln [A] - ln [A]0 = - kt Rearrange to the familiar form: ln [A] = - kt + ln [A]o