2) Below is a graph of reaction rate versus time. a. Identify where on the graph where the reaction reaches equilibrium. Explain your choice. b. What can you say about the forward reaction rate as time proceeds? c. What can you say about the reverse reaction rate as time proceeds? Reaction Rate vs. Time Data Set Reverse Reaction Rate Data Set 2 Forward Reaction Rate e 80- 60- 10 Time (min) 3) Below is a graph of concentration versus time. Identify on the graph where the reaction reaches equilibrium. a. Identify where on the graph where the reaction reaches equilibrium. Explain your choice. Concentration vs. Time Data Set. Products - Data Set 2:Reactant e 80- 60- 40- 20- 0- 0.0 20 4.0 Time (min) 6.0 80 Concentration (moVL) Reaction Rate (moVL "min)

2) Below is a graph of reaction rate versus time. a. Identify where on the graph where the reaction reaches equilibrium. Explain your choice. b. What can you say about the forward reaction rate as time proceeds? c. What can you say about the reverse reaction rate as time proceeds? Reaction Rate vs. Time Data Set Reverse Reaction Rate Data Set 2 Forward Reaction Rate e 80- 60- 10 Time (min) 3) Below is a graph of concentration versus time. Identify on the graph where the reaction reaches equilibrium. a. Identify where on the graph where the reaction reaches equilibrium. Explain your choice. Concentration vs. Time Data Set. Products - Data Set 2:Reactant e 80- 60- 40- 20- 0- 0.0 20 4.0 Time (min) 6.0 80 Concentration (moVL) Reaction Rate (moVL "min)

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter12: Kinetics

Section: Chapter Questions

Problem 11E: In the PhET Reactions under Options. (a) Leave the Initial Temperature at the default setting....

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In the PhET Reactions under Options. (a) Leave the Initial Temperature at the default setting. Observe the reaction. Is the rate of reaction fast or slow? (b) Click Pause" and then Reset All, and then enter 15 molecules of A and 10 molecules of BC once again. Select Show Bonds" under Options. This time, increase the initial temperature until, on the graph, the total average energy line is completely above the potential energy curve. Describe what happens to the reaction.
Provide the products (or reactants) and the names of the reactions when needed. Fast pls i will give u like for sure solve this question correctly in 5 min pls
In lab, a student obtained the following times for Mixtures 1-3. Using the solution concentrations from the lab manual, calculate the reaction order with respect to [ I − ] . Report your answer to two places after the decimal.Mixture Time (s)Mixture 1 14Mixture 2 36Mixture 3 44
I included my data table please answer the following questions Find the delta(S2O8^2-),M (2nd to last row on data table), THEN find the Reaction rate for all 4 runs (last row). IGNORE THE NUMBERS THAT ARE IN THOSE COLOUMNS RIGHT MOW THEY ARE MOST LIKELY INCORRECT! Next find the average rate consant k for the 4 runs using the numbers you calculated.
In lab, a student obtained the following times for Mixtures 1-3. Using the solution concentrations from the lab manual, calculate the reaction order with respect to [ I − ]. Report your answer to two places after the decimal. Mixture Time (s) Mixture 1 26 Mixture 2 32 Mixture 3 47 Flask 1, Mixture 1: KI 10mL, KCl 0mL, Na2S2O3 5mL. Flask 1, Mixture 2: KI 5mL, KCl 5mL, Na2S2O3 5mL. Flask 1, Mixture 3: KI 10mL, KCl 0mL, Na2S2O3 5mL. Flask 2, Mixture 1: (NH4)2S2O8 10mL, (NH4)2SO4 0mL Flask 2, Mixture 2: (NH4)2S2O8 10mL, (NH4)2SO4 0mL Flask 2, Mixture 3: (NH4)2S2O8 5mL, (NH4)2SO4 5mL KI, KCl = .2M (NH4)2S2O8, (NH4)2SO4 = .1M Na2S2O3 = .005M
I am learning reaction rates and my class is online. Could someone help me solve this table and show how to write out the calculations, I am super confused?
Reaction of interest : S2O82-(aq) + 3I- (aq)→ 2SO42-(aq) + I3-(aq). rate= k[S2O82-]1[I-]1.
Using graphical analysis program. Plot reaction time vs. concentration
The data below were determined for the reaction S2O82-(aq) + 3 I-(aq) ---> 2 SO42-(aq) + I3-(aq).Expt. # -----[ S2O82-]------- [I-]------ Initial Rate1 ............... 0.038 M .......0.060 M .....1.4 × 10- 5 M/s2 .................0.076 M .......0.060 M ..... 2.8 × 10- 5 M/s3 .................0.076 M .......0.030 M ..... 1.4 × 10- 5 M/s Which rate law is consistent with the experimental data for this reaction?
At the start of the reaction, the concentration of YOI is equal to 5.142 M. After 118.0 seconds, its concentration was reduced to 2.361 M. Meanwhile, another run of the same reaction but with 3.789 M [YOI]0 showed that after 110.0 seconds, a 1.350 M decrease in concentration of YOI was observed. Based on these: 1. How much YOI will be consumed if a run with [YOI]0 = 1.234 M is allowed to form MIYA for 4.00 minutes.
Create a procedure outline for calculating the activation energy of an iodine clock reaction, an example (this example has to do with determining rate equation for the clock reaction by measuring rates of reactions using different initial concentrations) : Measure reaction rate as a function of iodide I– concentration by decreasing initial iodide concentration while keeping all other concentrations constant. Use water to make up for volume loss for reduced amount of iodide stock solution. Measure reaction rate as a function of persulfate S2O 2– 8 concentration by decreasing initial persulfate concentration while keeping all other concentrations constant. Use water to make up for volume loss for reduced amount of persulfate stock solution. Use linear regression on log10 Rate as a function of log10[I– ]i or log10[S2O 2– 8 ]i for each reaction series to determine order for each reactant (exponent for the concentration in the rate law) Use measured rates, initial concentrations, and…
how reaction rate increases in pressure cooking because of collision theory and energy potential diagrams : how the rate of reaction is affected by temperature, surface area, nature of reactants, concentration, etc. by using collision theory? (use Hess’s Law, Le Châtelier’s Principle, or Kinetic Molecular Theory to explain in increasing rate of reaction and relevance by including all 4 required subtopics )