The activation energy of a certain reaction is 45.6 kJ/mol. At 20 °C, the rate constant is 0.0130 s-1. At what temperature would this reaction go twice as fast?Express your answer numerically in degrees Celsius> View Available Hint(s)T =SubmitPart BGiven that the initial rate constant is 0.0130s1 at an initial temperature of 20 °C. what would the rate constant be at a temperature of 100 "C?Express your answer numerically in inverse seconds.> View Available Hint(s)?k =Submit

A) We need to find temperature T2 B) We need to find rate constant K2

The activation energy of a certain reaction is 45.6 kJ/mol. At 20 °C, the rate constant is 0.0130 s. At what temperature would this reaction go twice as last? Express your answer numerically in degrees Celsius > View Available Hint(s) 阳 AE中 T2 = "C Submit Part B Given that the initial rate constant is 0.0130 s at an initial temperature of 20 °C, what would the rate constant be at a temperature of 100 °C? Express your answer numerically in inverse seconds. > View Available Hint(s) 1响AX中 k = s1 Submit

The activation energy of a certain reaction is 45.6 kJ/mol. At 20 °C, the rate constant is 0.0130 s. At what temperature would this reaction go twice as last? Express your answer numerically in degrees Celsius > View Available Hint(s) 阳 AE中 T2 = "C Submit Part B Given that the initial rate constant is 0.0130 s at an initial temperature of 20 °C, what would the rate constant be at a temperature of 100 °C? Express your answer numerically in inverse seconds. > View Available Hint(s) 1响AX中 k = s1 Submit

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 38QAP: Consider the first-order decomposition of phosgene at a certain temperature. COCl2(g)productsIt is...

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11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
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)?
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.
A catalyst reduces the activation energy of a reaction from 215 to 206 kJ. By what factor would you expect the reaction-rate constant to increase at 25 C? Assume that the pre-exponential term (A) is the same for both reactions. (Hint: Use the formula ln k = ln A Ea/RT.)
For the reaction AB+C, the following data were obtained at 30 C: [A] (M) 0.230 0.356 0.557 Rate (moI/L/s) 4.17104 9.99104 2.44103 (a) What is the order of the reaction with respect to [A], and what is the rate equation? (b) What is the rate constant?
Consider the first-order decomposition of phosgene at a certain temperature. COCl2(g)productsIt is found that the concentration of phosgene is 0.0450 M after 300 seconds and 0.0200 M after 500 seconds. Calculate the following: (a) the rate constant at the temperature of the decomposition (b) the half-life of the decomposition (c) the intial concentration of phosgene
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.