For protein X, you do not know the extinction coefficient of the substrate to calculate the true concentration. Therefore you are planning to calculate the initial rate of reaction as a change in absorbance per unit of time. After you did the experiment, you found that the the straightest portion of your graph is between 0 minute and 1 minute, and the absorbance changes from 0.865 to 0.132 within one minute. Calculate the initial velocity, which will be expressed as min-1.

For protein X, you do not know the extinction coefficient of the substrate to calculate the true concentration. Therefore you are planning to calculate the initial rate of reaction as a change in absorbance per unit of time. After you did the experiment, you found that the the straightest portion of your graph is between 0 minute and 1 minute, and the absorbance changes from 0.865 to 0.132 within one minute. Calculate the initial velocity, which will be expressed as min-1.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Given the following reaction and table of data, determine the rate law for this reaction: CH3X + 3X2 --> CX4 + 3 HX [CH3X] (M) [X2] (M) Initial Rate (M/s) 0.050 0.050 0.014 0.100 0.050 0.028 0.100 0.100 0.056 0.100 0.200 0.112 group of answer rate = k[CH3X][X2]2 rate = k[CH3X]2[X2] rate = k[CH3X] rate = k[CH3X][X2] rate = k[X2]
At noon time, the photochemical degradation of the DDT analogue DMDE has a rate constant of 0.8 h¹. Find the half-life (time for concentration of DMDE to decrease to 50% of the initial concentration value) for this reaction.
Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 1 0.250 0.340 0.0215 A + B → C + D 0.250 0.918 0.157 0.450 0.340 0.0387 Units k = DO IOL Teply 6:15 PM 5/3/2022 DELL End Delet Home Insert PrtScr F12 F11 F10 F9 F8 F7 F6 F5 F3 F4 Bac & 31
In a temperature-jump experiment to investigate the kinetics of an isomerization reaction that is first order in both directions, the relaxation time was measured as 27.6 μs. The rate constant for the forward reaction is known to be 12.4 ms–1. Calculate the rate constant for the reverse reaction.
A student ran a kinetics experiment on an unknown dye to determine the rate law. They plotted absorbance versus time (R 2 = 0.5472), LN(Absorbance) vs time (R 2 = 0.9979), and 1/Absorbance vs time (R 2 = 0.7680). Based on the R 2 values, what is the reaction order with respect to the dye in this student's experiment?
what is the activation energy? rate = r = k [I-]^1 [S2O82-]^1 Mixtures: Temperatures (celsius): Initial Rates: 1 21.9 6.45 * 10-4 2 38.9 3.54 * 10-4 3 2.4 4.35 * 10-4
show detailed work
Please help me, double and triple check your answers.
Given the following reaction and table of data, determine the rate law for this reaction: CH3X + 3X2 --> CX4 + 3 HX [CH3X] (M) [X2] (M) Initial Rate (M/s) 0.050 0.050 0.014 0.100 0.050 0.028 0.100 0.100 0.056 0.100 0.200 0.112 Group of answer choices rate = k[CH3X][X2]2 rate = k[CH3X]2[X2] rate = k[CH3X] rate = k[CH3X][X2] rate = k[X2]
There are several factors that affect the rate of a reaction. These factors include temperature, activation energy, steric factors (orientation), and also collision frequency, which changes with concentration and phase. All the factors that affect reaction rate can be summarized in an equation called the Arrhenius equation: KA-E/RT where is the rate constant, A is the frequency factor, Ea is the activation energy, R = 8.314 J mol-¹ K-¹ is the gas constant, and T is the absolute temperature. Figure In k slope= -1/T (K-¹) 1 of 1 ▼ Part A ▼ A certain reaction has an activation energy of 67.0 kJ mol-¹ and a frequency factor of A₁ = 3.80×10¹2 L mol-¹ s 1. What is the rate constant, k, of this reaction at 20.0 °C? k = Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash. Value Submit Request Answer Part B Units Y a is where y is In k, m is the slope or R' illustrated graphically in the image.…
The activation energy for the gas phase isomerization of cyclobutene is 136 kJ.(CH2)2(CH)2CH2=CHCH=CH2The rate constant at 429 K is 3.24×10-4 /s. The rate constant will be /s at 469 K.
In an enzyme-catalyzed 1st order process, a substrate has a half-life of 138 seconds. How long will it take for the substrate concentration to drop to 0.040 mmol/L if the beginning concentration is 1.28 mmol/L?