During a Michaelis Menten Kinetics experiment the following the standard curve and absorbance of one of the 5 min enzymatic reaction was obtained. • Calculate the initial velocity for the enzymatic reaction • Write a title for the standard curve and comment on the correlation between the standard curve data. 1.200 1.000 0.800 0.600 0.400 0.200 0.000 - Absorbance of enzymatic product (p-nitrophenol) y= 0.837x + 0.1182 R=0.9791 0.000 1.000 2.000 p nitropheol concentration absorbance

During a Michaelis Menten Kinetics experiment the following the standard curve and absorbance of one of the 5 min enzymatic reaction was obtained. • Calculate the initial velocity for the enzymatic reaction • Write a title for the standard curve and comment on the correlation between the standard curve data. 1.200 1.000 0.800 0.600 0.400 0.200 0.000 - Absorbance of enzymatic product (p-nitrophenol) y= 0.837x + 0.1182 R=0.9791 0.000 1.000 2.000 p nitropheol concentration absorbance

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

The following results were found after following the procedure Part B in the experiment: 0.053 M I- and 0.041 M H2O2 were used Temperature (oC) Calculated Reaction Rate (M/s) 12 0.031 30 0.119 88 0.797 Assuming the Rate Law = k[I-]2[H2O2] 2 Calculate the value of k at temperature 88oC. Give your answer to 1 place after the decimal.
help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working
An experiment was performed in a similar manner as Experiment 4 (The Hydrolysis of t-Butyl Chloride). The following data was obtained: Total Time (s) Volume NaOH Titrant used (mL) 46 2.01 91 3.97 131 5.98 175 8.03 220 10.00 266 11.99 311 14.01 357 15.97 401 17.98 450 20.02 Final Volume NaOH to fully react sample: 85.01 mL Assume the proposed reaction mechanism in the experimental procedure is correct. Based on the above measurements, how many minutes would it take for the solution to reach 81.0% completion? Round your final answer to two decimal places.
Ph OTs NaSCH₂ DMF NaCN DMSO Chem 240 Lab Activity 7: Reaction Mechanisms NaOMe MeOH
This is your graph. The rate of reaction at any point in time is given by the gradient of the concentration-time graph. Annotate your graph to show how you could determine the rate of reaction at 6 hours by drawing a tangent to the curve. Include your annotated graph in the answer and use the values from it to calculate the rate of reaction at 6 hours. Show your calculation in full.
Show structures of intermediate and write the reaction mechanism (include arrows and intermediates)
The rate of the second-order decomposition of ethanal (acet· aldehyde, CH3CHO) was measured over the temperature range 700-1000 K, and the rate constants are reported below. Find Ea and A.T/K 700 730 760 790kr/(dm3 mol-1 s-1) 0.011 0.035 0.105 0.343T/K 810 840 910 1000kr/(dm3 mol-1 s-1) 0.789 2.17 20.0 145
Please use the values in the resources listed below instead of the textbook values. The rate of the electron-exchange reaction between naphthalene (C10H8) and its anion radical (C10H8¯) in an organic solvent is diffusion controlled. C10H8 + C10H8 = C10H8 + C10H8 The reaction is bimolecular and second order. The rate constants are as follows. T/K 305 295 291 275 k/109 M-1.s-1 2.64 2.21 2.05 1.49 Calculate the values of Ea, AHº†, ASº† and AG°† at 295 K for the reaction. [Hint: Rearrange the equation below and plot In(k/T) versus 1/T.] KBT eASot/R@¬AH°†/RT(M1 – m) k = h Ea X kJ•mol-1 2993.386 AHo* X kJ•mol-1 2991.1 ASo# = X J:K-1.mol-1 -28069.52 AG°# X kJ•mol-1 107010.2
The mechanism proposed for the oxidation of iodide ion by the hypochlorite ion is shown below. Step 1 Step 2 CIO + H₂O I + HCIO HIO + OH HCIO + OH → HIO + CI (fast, equilibrium) This is reversible Step 3 IO + H₂O (fast) This is not reversible a. What is the overall reaction for this mechanism? Answer within the test and not on scratch paper. b. What are the intermediates if any are present? Answer within the test and not on scratch paper. c. What is the rate law expression for each step of the mechanism (including any reversible steps)? Answer this question on your scratch paper, clearly labeled. d. What is the predicted rate law expression for this reaction? Show all work to receive any credit. Answer this on your scratch paper, clearly labeled e. What would be the expected units for k using seconds for the time unit? Answer within the test and not on the scratch paper. (slow) This is not reversible
Please help, thanks.
You are now supplied with another set of results from a rate investigation, this time using reagents X and Y. Experiment Initial concentration of reactant X (mol dm-3) Initial concentration of reactant Y (mol dm-3) Relative rate 1 0.1 0.01 2 2 0.1 0.03 6 3 0.05 0.01 1 Write the rate equation for the reaction between X and Y. Show your reasoning. State the overall order of reaction. Give the units of the rate constant. Show your working clearly.
Calculate the time (min)required for a first-order reaction A -> Product to be 64.9% completed, knowing that the half lifetime t 1/2 is 206 min