03_ReactionRates_PostLab_Spring 24

0 State what rate law you would expect from this mechanism (Rate = k[Acetone]"[H*]"[[₂]') • Compare the expected rate law from the mechanism to the rate law you got from the Method of Initial rates and the Method of Isolation. If they are different, suggest 1-2 valid, specific, experimental reasons why they might be different. (fast, equilibrium) CH3 ソース H3C ག་ CH3 + H* = H3C H3C H. + H (slow) CH3 H3C CH2 + ↳2 Т + HI

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.

A + 2B -> C (rate constant = k1, rA = -k1[A][B]2) C -> A + 2B (rate constant = k-1, rA = k-1[C]) C + 2A -> 2D (rate constant = k2, rA = -k2[C][A]2) reaction rate constant and the rate for A of each elementary reaction are shown in the parentheses after each reaction.  Calculate the overall reaction rate for A in terms of [A], [B], k1, k-1, and k2   assuming c is psuedo-state-concentration  overall chemical rxn is 3A+2B->2D

Part A In this task, you'll observe a chemical reaction between baking soda and vinegar. How do temperature of the reactants and the rate of reaction are related? Write a hypothesis to predict the relationship between the two parameters. you think the в I U x² X2 15px E E E E E E r A A higher temperature of vinegar will make the reaction faster. Characters used: p2/ 15000 Part B Next, you'll test your hypothesis from part A by examining the reaction times of vinegar and baking soda in water at four different temperatures. You'll carry out the reaction using water at room temperature (about 25°C), 40°C, 60°C, and 80°C. Make sure that you use the same amounts of vinegar and baking soda for all three three trials. Gather all the materials, and perform these steps for each trial: 1. Heat at least cup (60 milliliters) of water to the required temperature (refer to the data table). Water may be heated on a stove, on a hot plate, or in a microwave oven. Measure and red he actual temnerature…

Answer 35 & 36 show-all-working-explaining-detailly-each-step Answer should be typewritten using a computer keyboard.

Your Task: Demonstrate how to determine the correct order of a reaction using your flowchart by explaining the path through the flowchart for one of the reaction orders (i.e. what are this queue or events (i.e. the relationship between the rate and the initial concentration, units on k, etc.) are you looking for. Imagine that you are writing to a classmate who doesn't yet understand the chemical kinetics. Thus, your microtheme will be judged not simply on whether or not your figure out the correct answer, but also on whether or not you can write clearly enough to teach a fellow classmate.

Use your experiment rate law and the average value for k to predict how long (in seconds)it would take for the acetone iodination reaction to finish for the initial conditions givenbelow. Note that you are solving for Δt in the average reaction rate.initial concentrations: [acetone] = 0.850 M[H+] = 0.320 M[I2] = 0.00150 Mreaction time (seconds): ______________How precise were the experimental measurements of the reaction time for each reactionmixture? How precise were the measurements of the value of the rate constant, k? Explain your answers.

Please don't handwrite  solution.

please help me answer a & b

The following mechanism has been proposed for the formation of N₂ and H₂O from H₂ and nitrogen monoxide Step 1 Step 2 2 NO N₂0₂ N₂0₂ (fast, equilibrium) This is reversible N₂0 H₂0 (fast, equilibrium) This is reversible Step 3 N₂ + H₂O (slow, RDS) This is not reversible a. What is the overall reaction for this mechanism? Answer this question within the test and not on the scratch paper b. What are the intermediates if my exist? Answer this question within the test and not on scratch paper. c. Write a rate law for sach step of the mechanism and list the molecularity of each step. Be sure to include any reversible steps as well. Answer this question on the scratch paper clearly labeled d. What is the predicted rate low for this reaction? Be sure to show all your work to receive credit. Arswer this question on the scratch paper clearly labeled. e. What are the expected units for k given the time in units of seconds. Answer this question within the test and not on the scratch paper,

Explain how the honeycomb structure affects the rate of the reaction at the molecular level. Use mini-CER format (3 sentences). Claim, evidence, reasoning.

hi, can you help me with a, b and c?

Plz do as soon as possible ....!

Directions: Determine the factor affecting the rate of reaction in the following statements. Write 1 for -concentration, 2 – for temperature, 3 - for surface area, and 4- for catalyst. 1. False denture cleaner tablet dissolves faster in water when in powdered form. 2. Bubbles were produced at faster rate in the test tube with hydrogen peroxide mix with manganese dioxide. 3. Japanese/crepe paper changes color with higher bleach solution. 4. Moderna vaccines require -70 to -80 degrees Celsius to maintain its efficacy rate. 5. Fever suspension medicines mix well with warm water. 6. More foamy substance is released when 3:1 mixture of baking soda and vinegar is made. 7. 20% HCI solution reacts faster when mixed with crushed than uncrushed egg shells. 8. Aluminum foil reacts with 30% muriatic acid diffusing gas all over the lab room. 9. Ozone depletes at a higher rate when sulfates are mixed with it. 10. Danger of explosion in places like coal mines is high because there are large qu ntids…

The reaction 2 N2O5(g) → 4 NO2(g) + O2(g) was studied and the rate of change of the concentration of O2 was found to be 3.65 mol L" 15-1. Correct! Calculate the reaction rate (in mol L1s1). Reaction rate = 3.65 mol L-1s1. eTextbook and Media Hint Attempts: 1 of 3 used Your Answer Correct Answer (Used) Calculate the rate at which N205 is consumed (in mol L1s1). d[N2O5]/dt = -7.30 mol L1s-1. Calculate the rate at which NO2 is formed (in mol L-s1). d[NO2]/dt = i mol L15-1. Save for Later Attempts: 0 of 3 used Submit Answer

Please explain the reaction mechanism and why it happens.

Main Content -Man Energy Reaction Progress RxnDiag21. Consider the reaction energy diagram provided. Which step in this reaction requires the least amount of activation energy? step one step two step three step four There is not enough information to determine this answer.

Direction: Determine whether the following statements conform to the rate law by writing True or False. _1. Rate law states that overall order of reaction can be determined by adding the reaction orders of the reactants. _2. Second order of reaction is the fastest. _3. All reactions proceed at the same rate. _4. The balance equation can be used to determine the rate of reaction. _5. The slow reactive or unreactive species in a reaction can be identified using rate law.

Please answer everything asap, I really need help.

Final Reactant Concentrations and Reaction Rates   [I-] [BrO3-] [H+] Reaction Time Rate of Reaction 2.8 x 10-5/time Expt. # M M M sec. M/sec 1 0.00166 0.0066 0.0166 258   2 0.0033 0.0666 0.0166 135   3 0.00166 0.0133 0.0166 132   4 0.00166 0.0066 0.033 78   FIND THE RATE?

Please show steps to solution with clear explanation.

of B → C is rate-determining. ● • Question 9: Write a rate equation for each reaction, given the indicated mechanism. a. CH3CH₂-Br + + OH b. (CH3)3C-Br slow (CH3)3C+ + Br CH,=CH, + H2O + Br -OH fast (CH3)2C=CH₂ + H₂O

Can someone help me solve this I'm completely lost

19. Predict the relative rates of these reactions. That is, select 1 next to the reaction with the fastest rate, 2 next to the reaction with the next fastest rate, and so onNote for advanced students: you may assume these reactions all take place in a polar aprotic solvent, like DMSO.

Chemistry How can I find the rate orders.

50 Concentration (mol/L) es Notes.pdf Reaction Rates Reaction rates are measured in units of which is = to 0.10 rate = Dnpoid 0.08- 1) Determine the average rate of product formation between 50 and 150 seconds. H90'0 0.04 2) Is the tangential slope positive or negative for: 0.02- - Product? reactant Reactant? 150 00, 250 Time (s) The at a single time is the rate. The slope over a range of time is the rate. Connection to Mathematics & Physics Slope is the rate of change. The symbol (delta) means "for a range (average rate of change). Example: A car decreases speed from 35 m/s to 15 m/s over a period of 5 seconds. What is the car's acceleration (average rate of change for velocity)? Example: The concentration of CHaF product increases from 0.20 mol/L to 0.80 mol/L over 12 seconds of reaction time. Determine the average reaction rate for this time. CH4 + F2 CH3F + HF

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III. Measuring the Rate of a Reaction Table GP.3: Reaction Rate Data Time (min) 0.00 0.25 0.50 0.75 1.00 1.25 1.50 Concentration of Phenyl Acetate (M) 0.54 0.44 0.32 0.22 0.16 0.12 0.082 a. Using Excel, prepare a graph of concentration vs. time using the data above. Make sure to show the best fit line for the data, the equation for the line, and the R2 value. Upload a picture or screen shot of your graph here. You can save your chart as a picture by right clicking on the chart and selecting "Save as picture". Do NOT upload an xls or xlsx file here.

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