Rate constants are temperature dependent. Therefore, the reactions must all be conducted at the same temperature in order for the linear relation derived above to be correct. Thus, another source of error in these experiments is any temperature difference between reaction flasks. Refer to the Introduction section where the identity of the rate-determining reaction was discussed. Suppose that the rate constant for reaction (1a) increases by 2% for each increase of 1 °C, and the rate constant for reaction (1b) increases by 20% for each increase of 1 °C. Q. What would be the percent decrease in the observed elapsed time when the temperature increases by 1 °C? 2% 20% O 2 + 20 = 22% 0.02 × 20 = 0.4%

Rate constants are temperature dependent. Therefore, the reactions must all be conducted at the same temperature in order for the linear relation derived above to be correct. Thus, another source of error in these experiments is any temperature difference between reaction flasks. Refer to the Introduction section where the identity of the rate-determining reaction was discussed. Suppose that the rate constant for reaction (1a) increases by 2% for each increase of 1 °C, and the rate constant for reaction (1b) increases by 20% for each increase of 1 °C. Q. What would be the percent decrease in the observed elapsed time when the temperature increases by 1 °C? 2% 20% O 2 + 20 = 22% 0.02 × 20 = 0.4%

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...

See similar textbooks

Similar questions

Let’s consider the following reaction, X+2Y - Z After performing some experiments, let’s assume a researcher has determined the rate law for this reaction to be, Rate = k [X][Y]2 But later, a second researcher reports that the mechanism for this reaction is actually, 2Y- 1 (slow) X+1- Z (fast) In the previously determined rate law consistent with this mechanism? If not, why? What should be rate law predicted by this mechanism?
For the following reaction of protein dimerization, 2P P. the concentration of protein monomer, P, in the aqueous solution at time zero was 0.2x10 mol L and at time 200 s the concentration was 0.02x10 3 mol L1. Calculate the reaction rate constant k. Select the closest value. 225 s-1 mol L-1 O 5s1 mol1 L O0.5 s1 mol1 L2 O 0.02 s1 mol L·1 O 14.6 s´1 mol L GD 53 s1 mo1 O53x 10 s1 mol 2 0.24 x 10 s1 mol 2
(2) The reaction-rate data given below were obtained using a batch reaction system for the reaction A→products. Plot the data in appropriate form to test the fit for zero- and first-order kinetics. From the plot that gives the best fit, determine the appropriate reaction rate constant (remember the units). Time, min CA, (g/m3) 0 30 0.5 25.4 1 21.6 2 16.9 4 13.1 8 8.3 16 3.2 32 0.31
The overall gas phase reaction 3A --> B + 2C occurs via the following sequence of elementary steps 2A <--> I1 + B k1,k2 A + I1 --> 2I2 k2 I2 --> C k3 1. write an expression for the overall reaction rate, r, in terms of the rate step 3, r3 2. using the answer from 1, obtain an expression for the reaction rate, r, in terms of rate constants and concentrations of reactants and products, only use PSSH. 3. State the. specific inequality the must be satisfied for each of the following assumptions to hold, and use it to simplify the general rate expression from question 2. i) Step 1 is quasi-equilibrium ii) Step 1 is irreversible
(3) Evaluate the following uses of catalysis in terms of the goals of green chemistry (it is up to you if you want to refer to the 12 Principles or just the more general goals proposed by Dr. Lipke). Identify benefits as well as possible downsides. 2 a. A catalytic process that uses O, to oxidize an organic substrate dissolved in hexanes as a solvent, replacing a previous process that required the use of pyridine-N-oxide as an oxidant. b. A catalytic process that allows organic plant matter to be broken down into small organic molecules that can be used to produce fuels and fine chemicals that would otherwise be made from petroleum. c. A catalytic process that uses a mercury salt to catalyze the oxidation of methane to a methanol derivative, circumventing 2 a more traditional route using H, and CO to produce methanol as an intermediate.
Q6. Does the Rate Constant for the reaction between Parts B and C have the same value or are they different. Briefly explain your answer. Note: You do not need to carry out a calculation to answer this question
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
3) A chemical reaction was conducted at 4 different temperatures and the following data was obtained. Plot the In(k) versus the inverse of the respective temperature using linear regression analysis (Excel). Find the slope (from the graph) and what does that number represent? Use Arrhenius equation. Calculate the Activation Energy for the reaction. Rate constant (k) Temperature of reaction (°C) 0.0521 15 0.101 25 0.184 35 0.332 45 NOTE: Make sure to attach the graph paper with proper calculation.
Use the data given below to find rate constant. Then derive the rate law for this reaction. Show your work in a separate sheet. S20g2-(ag) + 31(ag) 2 SO42-(g) +13 (a4) [S20g2-i (M) [[h (M) Initial Rate (M/s) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33 Rate = [36 M -1s-1IS 20 8 2-1] [86 M -25-1S 20 82-12 Rate = Rate = [120 M -25-1S 20 82121] Rate = [195 M -3s 1S 20 8 21211-2
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.
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.