The activation energy of an uncatalyzed reaction is 86 kJ/mol. The addition of a catalyst lowers the activationenergy to 81 kJ/molPart AAssuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 24 °C?Express the ratio to two significant digits.Templates Symbols undo rego feset keyboard shortcuts Helpk./k, = 23•106SubmitPrevlous Anawers Requeat AnawerX Incorrect; Try Again; 7 attempts remainingPart BAssuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 128 °C?Express the ratio to two significant digits.Templates SymBols undo redo Teset keyboard shortcuts Helpk/k =SubmitRequest Anewer< Return to AssignmentProvide Feedback

Given data :- Activation energy of uncatalyzed reaction (ENC) = 80 kj/mol = 80000 J/mol Activation…

The activation energy of an uncatalyzed reaction is 86 k.J/mol. The addition of a catalyst lowers the activation energy to 81 kJ/mol • Part A e of the reaction at 24 "C? Assuming that the colision factor remains the same, by what factor will the catalyst increase the Express the ratio to two significant digits. Templates Symbols undo redo feset keyboard shortouts Help k. /k. - 2.3 • 10° Submit Previous Answer Request Answer X Incorrect; Try Again; 7 attempts remaining • Part B Assuming that the colision factor remains the same, by what factor will the catalyst increase the e of the reaction at 128 "C? Express the ratio to two significant digits. Templates Symbol undo rego feset keyboard shortouts Help k. /k. =

The activation energy of an uncatalyzed reaction is 86 k.J/mol. The addition of a catalyst lowers the activation energy to 81 kJ/mol • Part A e of the reaction at 24 "C? Assuming that the colision factor remains the same, by what factor will the catalyst increase the Express the ratio to two significant digits. Templates Symbols undo redo feset keyboard shortouts Help k. /k. - 2.3 • 10° Submit Previous Answer Request Answer X Incorrect; Try Again; 7 attempts remaining • Part B Assuming that the colision factor remains the same, by what factor will the catalyst increase the e of the reaction at 128 "C? Express the ratio to two significant digits. Templates Symbol undo rego feset keyboard shortouts Help k. /k. =

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 71QAP: For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation...

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For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
Experiments during a recent summer on a number of fireflies (small beetles, Lampyridaes photinus) showed that the average interval between flashes of individual insects was 16.3 s at 21.0C and 13.0 sat 27.8C. a. What is the apparent activation energy of the reaction that controls the flashing? b. What would be the average interval between flashes of an individual firefly at 30.0C? c. Compare the observed intervals and the one you calculated in part b to the rule of thumb that the Celsius temperature is 54 minus twice the interval between flashes.
Compare the functions of homogeneous and heterogeneous catalysts.
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay. HCOOH(g) CO2(g) + H2(g) At 550 C, the half-life of formic acid is 24.5 minutes. (a) What is the rate constant, and what are its units? (b) How many seconds are needed for formic acid, initially 0.15 M, to decrease to 0.015 M?
What is the difference between average rate, initial rate, and instantaneous rate?
The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
Show how equation 20.33 reduces to a simpler form of an integrated first-order rate law when the reverse reaction of an equilibrium is negligible.
Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, fur the reaction was measured at several different temperatures and the data are shown here: Temperature (K) k (M -1 5-1) 555 6.23107 575 2.42106 645 1.44104 700 2.01103 What is the value of the activation energy (in kJ/mol) for this reaction?
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
A substance undergoes first-order decomposition. After 40.0 min at 500°C, only 12.5% of the original sample remains. YYliat is the half-life of the decomposition? If the original sample weighed 243 g, how much would remain after 2.00 h?
A study of the rate of the reaction represented as 2AB gave the following data: Time (s) 0.0 5.0 10.0 15.0 20.0 25.0 35.0 [A](M) 1.00 0.775 0.625 0.465 0.350 0.205 0.230 (a) Determine the average rate of disappearance of A between 0.0 s and 10.0 s, and between 10.0 s and 20.0 s. (b) Estimate the instantaneous rate of disappearance of A at 15.0 s from a graph of time versus [A]. What are theunits of this rate? (c) Use the rates found in parts (a) and (b) to determine the average rate of formation of B between 0.00 s and 10.0 s, and the instantaneous rate of formation of B at 15.0 s.