pre lab 3 chem 2

1. This question is adapted from Harris 19-D. Carnosine is a dipeptide whose antioxidant properties protect cells from free radicals. Carnosine was determined by derivatization with naphthalene-2,3-dicarboxyaldehyde and cyanide followed by fluorescence detection using excitation at 445 nm and emission at 490. Quantification was by standard addition. To four aliquots of 20-ul cell lysate were added volumes of 100µM carnosine standard to generate final concentrations of 0, 1.0, 2.5, and 5.0 µM added carnosine. Solutions were diluted to 70µl before addition of 15µl of 5 mM naphthalene-2,3-dicarboxyaldehyde and 15µl of 10 mM NaCN. H H2N. OH Carnosine HN. Naphthalene-2,3- dicarboxyaldehyde Cyanide OH Fluorescent product HN. Fluorescence intensity Concentration (uM) of added carnosine in final 100 µL 0.0 0.465 1.0 0.698 2.5 1.029 5.0 1.651

Task 2. Order of reaction Direction: Answer the following questions. Show your solutions. A. Initial rates for the reaction of nitrogen monoxide and chlorine 2NO(g) + Cl₂2 (g) → 2NOCI(g) were measured at 27°C starting with various concentrations of NO and Cl₂. These data were collected. Initial Concentration (mol/L) [NO] [Ch] 0.020 0.010 Experiment 1. 8.27 x 10-5 1.65 x 104 3.31 x 10-4 6.60 x 10-4 5 0.010 0.020 4.10 10.5 What is the order of the reaction with respect to each reactant, the overall order of the reaction, and its rate law? 2 3 ترا 4 0.020 0.020 0.040 2. What is the value of the rate constant k? 0.020 0.040 Initial Rate (M/s) 0.020

I got #8a correct, but #8b is incorrect and I can’t figure out why? Please help.

Plot a Graph and Determine the Rate: Make a graphical plot of reaction time (x-axis) and spectrophotometer readings [Use the calculated average] (y-axis). Determine the initial velocity (rate) of the reaction by extending the initial straight-line portion of your reaction curve and calculating the gradient of the straight line (difference in y/ difference in ×). The units of the rate will be in absorbance units min' (abs min-"). What is the rate of the reaction based on your plotted values:

Plot a Graph and Determine the Rate: Make a graphical plot of reaction time (x-axis) and spectrophotometer readings [Use the calculated average] (y-axis). Determine the initial velocity (rate) of the reaction by extending the initial straight-line portion of your reaction curve and calculating the gradient of the straight line (difference in y/ difference in ×). The units of the rate will be in absorbance units min' (abs min-"). What is the rate of the reaction based on your plotted values:

Answer question 3

4

Explain how changing Experimental Volume impacted the kinetics of the reaction. Compare to your prediction. Be concise. ( in short sentence)

PERTINENT CALCULATIONS Remember: rate = k[C25H30CIN3]"[OH_]" where n =0 since excess OH was used. n3= 1. Refer to your graphs and complete table below Linear correlation (r- value) Graph Kinetic Run I Kinetic Run II Average r- value absorbance vs time 0.9972 0.9955 0.9964 In (absorbance) vs time 0.9978 0.9994 0.9986 2/(absorbance) vs time 0.9805 0.9879 0.9952 2. Based on the average linear correlation (r2 -value) the reaction order, m, with respect to crystal violet, CV, is Explain. 3. Write the rate law. 4. The slope, and therefore pseudo" rate constant, kr', is at T1. CC, and ko' is at T2

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Pre-lab questions 1. The stock concentration values cannot be used as the initial concentrations for the calculation of the reaction rate. Briefly explain. 2. Using these data, determine the order of reaction with respect to reactant A. A + B + C+ D Trial #1 Trial #2 Trial #3 [A], M [B], M 0.16 0.32 0.16 0.16 0.08 0.16 Rate, M/s 4.0x10* 8.0x10* 1.6x10* 3. Determine the order of reaction with respect to reactant B. 4. Calculate the rate constant for this reaction of A and B.

Using the graph below, determine the time it will take for half of the reagent present at t = 60 sec to react. b.  196 s c.  256 s d.  120 s e.  60 s

1- In the enzymatic reaction that took place in the batch constant volume reactor, the reaction rates were measured at different initial concentrations and are given in the table below. Find the appropriate kinetic model and coefficients Substrate cconcentration (mM) 1 2 4 16 32 Reaction rate (mmol/L min) 1 1.8 3.2 6.6 7.8

Ps. This is not graded.

What is m and n

please show work or why you chose that answer   thankyou so much!

Having a hard time with how to determine reaction rate

the mean time, the rate, [S₂O3] in the reaction may label clear outliers the mean) as such and e calculation. on mixtures NH4)2SO4 (NH4)2S2O8| (mL) (mL) 1.50 0.50 1.50 0.50 1.00 1.00 1.00 1.00 following reagents are um iodide ium persulfate m thiosulfate um nitrate ium sulfate odide in the solution in the Answer: 0.050 M • Determination of the rate law follows the protocol in ref. (5). with one difference. A reactant order (rate law exponent) will be calculated twice using two different pairs of determinations (e.g. determinations 1 & 2 and determinations 3 & 4). Then the mean is taken of both values and reported as order. This is done for each reactant. This additional step allows us to include more data and reduce experimental error. Practice Problem 2: The rate of a reaction CO(g) +3H₂(g)→ CH4(g) + H₂O(g) was determined at 25 °C. From the following data, determine a) the mean reaction order with respect to CO b) the mean reaction order with respect to H₂ c) the overall rate order d)…

You continue with the Arrhenius Plot with the slope of the curve to be approximately -12,500 K and the Arrhenius factor of 4.367 E10 hours^-1. What is the shelf life of the drug at 22 C? What is the shelf life at 4 C? Be sure to show your calculations. Arrhenius Plot -8 -10 -12 -14 -16 -18 0.0026 0.0028 0.0030 0.0032 0.003 1/T In (k)

Run Reactants Temperature (Celsius) Initial Rate (kPa/s)   1 10 ml 3% H2O2 = 5ml 0.5M KI 23.0 0.0798 2 5ml 3% H2O2 = 5ml 0.5 M KI 23.0 0.0391 3 5ml 3% H2O2 + 10ml 0.5 M KI 23.0 0.0794     Run Initial Rate (mol/L*s) [H2O2] after mixing [I-] after mixing 1 3.24 x 10^-5 0.147 M 0.0417 M 2 1.59 x 10^-5 0.0733 M 0.417 M 3 3.23 x 10^-5 0.0733 M 0.0833 M   Calculate the rate law for the reaction

B IU Av A 1. Using the Ideal Gas Law (PV = nRT), calculate the grams of O2 produced in the reaction. Show %3D your work and follow the steps below. If you pressure is not yet in atm, convert it to atm using the appropriate conversion factor. b. Convert the volume of oxygen collected from mL to L. C. Convert the temperature of the water from °C to K. d. Plug in P, V, R (gas constant), and T to the ideal gas law and solve for n, which is moles of oxygen gas. e. Use the moles of oxygen gas found and the molar mass of O2 to calculate the grams of oxygen produced using dimensional analysis.

L Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. Elementary Step 1 H+ + H₂O₂ = {H₂O*- OH) (rapid equilibrium) Elementary Step 2 (H₂O*-OH) + Br¨ → HOBr + H₂O (slowest) Elementary Step 3 HOBr+ H+ + Br¯ → Br₂ + H₂O (fast) Consider the reaction profile below. What is the approximate activation energy (Ea) for elementary step 2? 7

How was Thin Layer Chromatography (TLC) used in organic synthesis reactions ? TLC is used to find the exact concentration of a catalyst in the reaction. TLC can speed up a reaction because silica gel is polar. TLC can separate components of a reaction mixture such as starting materials and products allowing the experimenter to identify what compounds are in the reaction mixture. TLC is used to find percentage yield of the reaction.

Plot on to graph moles of S2O8 vs time to achieve M/s. The initial concentration of S2O8: 0.05M (added is 2.5mL of 0.200M, but it was diluted so 0.200 x 2.5/10mL = 0.05M).  Below is the time (s) and moles consumed. 188s - 0.00002 moles 362s - 0.00004 moles 548s  - 0.00006 moles 740s - 0.00008 moles 1001s - 0.0001 moles I was told to plot concentration vs time then subtract the moles, but I'm confused how to do that.

Pls help ASAP. Pls show all work.

What are limitations and improvements in this experiment and source of errors

Pls help on this ASAP. Pls do with all steps.

You are trying to determine the KM for an enzyme. Due to a lab mishap, you have only two usable data points: Use these data to calculate an approximate value for KM. Is this value likely to be an overestimate or an underestimate of the true value? Explain.

1. Determine the concentration of each component (C2) in the final mixture for each run (refer to Table 4-1) for the total volume (V2) of the mixture, and the initial concentration (C1) and volume (V1) of each component). C1V1 = C2V2 2. Calculate for the reaction rate per run using the concentration of iodine and time elapsed. reaction rate = [I2] in the final mixture/time elapsed 3. Determine the reaction order with respect to l2. Also determine the reaction order with respect to C3H6O and the reaction order with respect to HCI. Round off your answers to the nearest whole number. 4. Calculate for the rate constant for each run using the reaction orders obtained (use rounded off values of reaction orders). 5. Take the average of the rate constants. 6. Determine the rate law of the reaction.

A learning.mheducation.com Types of Reactions assignment and quiz F. Question Mode: Multiple Select Question Explain the different types of chemical react... https://moodle.coastal.edu/pluginfile.php/106... https://moodle.coastal.edu/pluginfile.php/106... Exit Assignment X Mc Graw Hill 13 of 36 Concepts completed i Multiple Select Question Select all that apply LI Which of the following reactions are expected to occur as written, with Ba reference to the activity series for metals (shown)? Select all that apply. Ca O Cu (s) + 2HCI (aq) → CuCl2 (aq) + H2 (g) Na Mg Mg (s) + Co(NO3)2 (aq) → Co (s) + Mg(NO3)2 (aq) Al Mn O Pb (s) + 2HCI (aq) → PbCl2 (s) + H2 (g) Zn Cr O 3Ag (s) + Fe(NO3)3 (aq) → 3ÄGNO3 (aq) + Fe (s) Fe NI Sn Pb H2 Cu Hg Ag Au Copyright O McGraw-Hll Education EText Alternative Need help? Review these concept resources. E Reading Rate your confidence to submit your answer. High Medium Low O2021 McGraw-Hill Education. All Rights Reserved. Privacy Terms of Use 80 888 DII DD F10…

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!

how do you divide the rate expression for Trial 2 by that for Trial 1 and simplify? How do you solve for a?