step 1 fast: 2 OF,=0;F4 step 2 slow: 0,F1→02+2 F, (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"[B]"... , where '1' is understood (so don't write it if it's a 'l') for m, n etc. Rate =

step 1 fast: 2 OF,=0;F4 step 2 slow: 0,F1→02+2 F, (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"[B]"... , where '1' is understood (so don't write it if it's a 'l') for m, n etc. Rate =

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...

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how is “rate law expression” and “rate determining step” different?
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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.
KINETICS AND EQUILIBRIUM Expressing the concentration of an intermediate in terms of the... Consider the following elementary reaction: IC1(g) +H₂(g) →HI(g) + HCl(g) Suppose we let k₁ stand for the rate constant of this reaction, and k_₁ stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of HI in terms of k₁, k-1, and the equilibrium concentrations of IC1, H₂, and HC1. [HI] = 0 X 3/5
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
The starting concentration (time zero) of crystal violet is 1 x 10-4 M. Using the proper integrated rate law and the calculated value for k, calculate the concentration of crystal violet after 240 seconds. Look at the equation of the trend line for your lost linear graph and the beer-lambert law. Equation from graph from NaOH 0.0660M is y= -0.0105x-0.6277
Consider the following elementary reaction: (g) (g) Suppose we let stand for the rate constant of this reaction, and stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of in terms of , , and the equilibrium concentration of .
A student follows the Determining the Rate Law for the Crystal Violet-Hydroxide lon Reaction procedure. The stock concentration of sodium hydroxide used in trial 1 is 0.020 M. The stock concentration of sodium hydroxide used in trial 2 is 0.010 M. After graphing the data, the slope of the straight-plot line for trial 1 is -0.0722 and for trial 2 is -0.0712. Calculate the reaction order with respect to hydroxide ion concentration. Give your answer as an integer.
A reiction is described as follows: 2A (g) + 2B (g) -+C (g) Exp. (A). M Initial rate (x10* Ms') 0.15 0.15 0.15 1.24 2.46 4.95 2. 032 0.15 3 0.30 From the data given above, determine the followings: (1) The rate law formula in terms of formation of product C, (ii) The overall order and the order with respect to each component, (ii) The rate constant (state clearly its units and coefficients), (iv) Find the rate of reaction when (A] - [BI =0.20 M.
tab esc slock ||| = OKINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism with an initi.... Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) + O₂ (g). -NO₂(g) + O₂(g) k₁ 2 NO₂ (g) + NO₂ (g) → N₂O5 (g) k₂ Suppose also k₁ «k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. BE 1 Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Explanation Q A @ 2 Check W S X # 3 E 0 rate = k 14 D $ 4 rate constant > R F % 5 © Stv T MacBook Pro 6 G We Y & 7 H 0-0 U 00 Ⓒ2022 McGraw Hill LLC. All R You * 00 00 8 S a (
Please solve correctly, find value of x,y,z
Answer the following questions from number 2 up to 5.