Lab 4 Chm Kinetics Part II Prelab Questions

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

ew K History Bookmarks DZL Rate Laws Expe X Profiles Tab Determination c X 1 Homework 2 ttempt 1 Listen Window my.edu/d21/le/content/408344/viewContent/17004406/View Help Your Answer: Rates Law Expe X D21 4. CLASS SLIDE X 3 What is the rate constant for a reaction based on the following experimental information? Expt Rate (M/s) [A] (mol/L) [B] (mol/L) 1 0.5170 0.700 0.648 2 1.4912 1.189 0.648 1.2205 1.529 D21 Activity Assignr X 0.700 Report your answer to THREE significant figures. A ALEKS-Isabell x E

1. Factors Affecting Reaction rate 1A. Effect of Reactant Concentration Test Concentration Observation Initial Final Total Tube # of HCI Time Time Time Slow evolution of colorless gas, Fast evolution of colorless 0 sec O sec 17 min 1 1.0 M 5 sec 4 min 2.0 M 38 sec gas Very fast evolution of colorless gas O sec 1 min 20 sec 3 3.0 М 2.

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Values if needed for this question. The following initial rate data are for the reaction of mercury(II) chloride with oxalate ion: 2 HgCl2 + 2 CI + Hg,Cl2 + 2 CO2 Experiment [HgCl2]o, M [C,0,?], M Initial Rate, M sl 1 0.415 0.180 1.23x104 0.830 0.180 2.45x104 4.91×10-4 9.81×104 3 0.415 0.360 4 0.830 0.360 Complete the rate law for this reaction in the box below. Use the form k[A]™[B]" , where '1' is understood for m or n and concentrations taken to the power not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M2s1 Submit Answer Try Another Version 2 item attempts remaining

Reaction kinetics lab Can anyone help me to answer the question please?

A student determines the time required for 10% reaction by the method described in part A of the procedure of this experiment. She records a time of 45.6 seconds for trial 1, 40.2 seconds for trial 2, and 40.4 seconds for trial 3. a. b. c. Calculate the average time (in seconds) required for 10% reaction. Calculate the average rate (in M/s) required for 10% reaction. Calculate the rate constant, k, (in s^-1).

Chemistry How can I find the rate orders.

MISSED THIS? Read Section 15.5 (Pages 650-656). The following data show the rate constant of al reaction measured at several different temperatures. Temperature (K)Rate constant (1/s) 300 310 320 330 340 0.197 0.561 1.50 3.77 8.98 Use an Arrhenius plot to determine the activation barrier (E) for the reaction. Express your answer using three significant figures. 15. ΑΣΦΑ E₁= Submit Part B Request Answer ww kJ/mol PEC Review Use an Arrhenius plot to determine the frequency factor (A) for the reaction. Express your answer using two significant figures. ΞΑΣΦΑ 8 1

What are relevant chemical concepts, ideas and theories of this experiment

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Using data from Part B, quantitatively explain how the magnitude of the rate changes with the reactant concentration.

1. indicate the activation energy for the overall reaction on the graph. (You may want to use a line for the sake of clarity.)2. Write the elementary reactions that make up the reaction mechanism. 3. What would you propose as the rate law for this reaction? 4. Of course, this proposed law is hypothetical. Using the following data collected experimentally (probably using a UV/vis spectrometer J), determine the rate law for this reaction. Include reaction order and the value and units for k. Please show your work, including any graphs you make. (Note: no credit will be given to correct final answers without supporting work.) Does your experimental rate law match the one you proposed above?

When fitting data to a best fit line, a correlation coefficient (R2) is determined and used to evaluate the quality of fit. The best fit of the data will have an R² value closest or equal to zero (0). closest or equal to one (1). equal to the rate of the reaction occurring. equal to the rate constant of the reaction occurring.

I need to find the rate law to fill in the chart shown. Table 1-Initial moles The concentrations for all three stock solutions are given at the top of the data sheet. The volumes used for each experiment are in chart 1 on the data sheet.   Convert the volumes from mL to L using the metric system. Multiply the volume (L) by the molarity to determine the initial number of moles for each substance.

1.Write the rate equation for the reaction between X and Y. Show your reasoning. 2.State the overall order of reaction. Give the units of the rate constant. Show your working clearly. 3. The initial rate is 1.25 x 10^-3 moldm^3s^-1 . calculate the value of the rate constant for the reaction under the conditions of the experiment

please. helpp. this unit is about chemical kinetics. PLEASEE ANSWER BOTH AS THEY ARE PART OF 1 QUESTION ONLY. I REALLY NEED HELP

The OH radical disproportionates in gas phase according to the elementary reaction: OH + OH → H20 + O. At [OH]o =1 µM, the initial rate of water formation is 1019 molecules per 1 cm3 per second. What is a rate constant of this bimolecular reaction in M-'s-1? Select one: a. 4.15*109 b. 1.26*108 c. 2.15*109 d. 1.66*1010 e. 1.45*1011

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