On the other hand, the order in respect to 〖[OH〗^-] would have been found by using the observed rate constants, which are the negated slope values for the plots ln(abs at 595nm) versus time. As stated, since the data recorded from run 2 is not reliable, the observed rate constant was not used for calculations. Therefore, the accepted value of ‘one’ was assumed, making the order with respect to OH^- one. With the order of both crystal violet and hydroxide found to be first order, with an overall reaction order of two, the rate law for the reaction of crystal violet with hydroxide is found to be equation 9, Rate=k[C〖V]〗^1 …show more content…
The true rate constant for the overall reaction, k, does not depend on hydroxide’s concentration and will remain constant regardless of the concentration. On the contrary, the rate constant is dependent on temperature; therefore, the temperature must be kept the same throughout the experiment. The observed rate constant and true rate constant had units of s^(-1) and M^(-1) s^(-1), respectively. The units for both the observed rate constant and true rate constant were found with the use of equation 8 and 9. (With the knowledge obtained that crystal violet is a first order reaction and the accepted value of “one” for y, making hydroxide a first order reaction, as