n Experiment 2, you will study the kinetics reaction of crystal violet, CV+, an intensely colored acid-base indicator that decolorizes in the presence of a large excess of base. The reaction will be monitored colorimetrically, by measuring the absorbance, A, of the solution as a function of time.
Absorbance
Time
0.480 0
0.439 211
0.385 527
0.349 756
0.332 879
0.320 967
0.304 1090
he above data were measured under the conditions: [OH-] >> [CV+].
Deduce the order of the reaction with respect to [CV+], by determining which relationship is most nearly linear.
Calculate the pseudo rate constant, k1', using the slope of the appropriate linear regression line.
i tried differents excel spreedshit but i couldont get the right answer
any help appreciated
Absorbance
Time
0.480 0
0.439 211
0.385 527
0.349 756
0.332 879
0.320 967
0.304 1090
he above data were measured under the conditions: [OH-] >> [CV+].
Deduce the order of the reaction with respect to [CV+], by determining which relationship is most nearly linear.
Calculate the pseudo rate constant, k1', using the slope of the appropriate linear regression line.
i tried differents excel spreedshit but i couldont get the right answer
any help appreciated
-
Spread "****" is right ;-)
Actually, I tried this series and got an exact fit (R^2 = 1) using an exponential curve. The equation is y = 4.80E-01 * e^-4.19E-04x. Generally an exponential decay indicates a first-order reaction.
The pseudo first order rate constant k1' is the exponent, -4.19E-04 (that is, 0.000419). The unit is s^-1 since x is in seconds.
Actually, I tried this series and got an exact fit (R^2 = 1) using an exponential curve. The equation is y = 4.80E-01 * e^-4.19E-04x. Generally an exponential decay indicates a first-order reaction.
The pseudo first order rate constant k1' is the exponent, -4.19E-04 (that is, 0.000419). The unit is s^-1 since x is in seconds.