A second-order reaction has a rate constant of 9.7 × 10 /(M • s) at 30.°C. At 40.°C, the rate constant is 3.1 × 10-3 /(M • s). What are the activation energy and frequency factor for this reaction? Predict the value of the rate constant at 45°C. Activation energy = | kJ/mol Frequency factor· /(M • s) Rate constant /(M · s)

A second-order reaction has a rate constant of 9.7 × 10 /(M • s) at 30.°C. At 40.°C, the rate constant is 3.1 × 10-3 /(M • s). What are the activation energy and frequency factor for this reaction? Predict the value of the rate constant at 45°C. Activation energy = | kJ/mol Frequency factor· /(M • s) Rate constant /(M · s)

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

The rate of a certain reaction was studied at various temperatures. The table shows temperature (7) and rate constant (k) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, Ea, for this reaction? E₂ = What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction? A = kJ. mol-¹ $ $1 T(K) 400 420 440 460 480 500 520 540 560 580 k (s-¹) 0.000369 0.00200 0.00928 0.0377 0.136 0.445 1.33 3.64 9.31 22.3
In a series of experiments on the decomposition of dinitrogen pentoxide, N2O5, rate constants were determined at two different temperatures. At 35°C, the rate constant was found to equal 1.4x10-4/s and at (4.20x10^1)°C the rate constant was 5.0x10-4/s. What is the activation energy, in J/mol, for this reaction? Express your answer to three significant figures.
There are several factors that affect the rate constant of a reaction. These factors include temperature, Templetes activation energy, steric factors (orientation), and also collision frequency, which changes with concentration and phase. All the factors that affect the rate constant can be summarized in an equation called the Arrhenius equation: Part A k= Ae/r where k is the rate constant, A is the frequency factor, E, is the activation energy, R= 8.314 J/(mol - K) is the universal gas constant, and T is the absolute temperature. A certain reaction has an activation energy of 70.0 kJ/mol and a frequency factor of A1 = 6.10x1012 M-'s 1. What is the rate constant, k, of this reaction at 29.0 °C ? Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash. > View Available Hint(s) Tempjetes Symbols undo redo test keyboard shortouts Help k= 1.61 m's-1 Submit Prevlous Anawere X Incorrect; Try Again;…
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=17.0 kJ/mol. If the rate constant of this a - 1 reaction is 8.5 × 10° M - 1 S. at 156.0 °C, what will the rate constant be at 225.0 °C? Round your answer to 2 significant digits. - 1 - 1 k = [] M ¯' . •S ?
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 54.0 kJ/mol. If the rate constant of this reaction is 2.0 × 10³ M¹s -1.-1 at 222.0 °C, what will the rate constant be at 272.0 °C? Round your answer to 2 significant digits. k = M .S Ś 囧

Be sure to answer all parts. The first-order rate constant for the reaction of methyl chloride (CH3CI) with water to produce methanol (CH,OH) and hydrochloric acid (HCI) is 3.32 x 10-10s at 25°C. Calculate the rate constant at 45.1°C if the activation energy is 116 kJ/mol. x 10 (Enter your answer in scientific notation.) DELL F10 F11 F12 Pr F7 F8 F9 F4 F5 F6 144
References] Calculate the activation energy, Ea, for the reaction 2 N₂O5 (g) →4 NO2(g) + O2(g) from the observed rate constants: k at 25 °C 3.46 x 105 s¹ and k at 53 °C 1.20 x 10-3 s¹. The gas constant R is 8.3145 x 10³ kJ/mol. K. = kJ/mol
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=64.0 kJ/mol. If the rate constant of this -1 reaction is 0.0021 M - 1 S. at 40.0 °C, what will the rate constant be at -32.0 °C? Round your answer to 2 significant digits. 1 |M - 1 k = •S Ox10
A second-order reaction has a rate constant of 7.7 x 10- /(M s) at 30.°C. At 40.°C, the rate constant is 2.6 x 10 (M s). What are the activation energy and frequency factor for this reaction? Predict the value of the rate constant at 45°C. Activation energy = KJ/mol Frequency factor - (M s) Rate constant = /(M s)
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=69.0 kJ/mol. If the а - 1 rate constant of this reaction is 5.7 × 10² M - 1 S. at 304.0 °C, what will the rate constant be at 256.0 °C? Round your answer to 2 significant digits. - 1 - 1 k = || M •S x10 ?
The activation energy of a certain reaction is 41.8 kJ/mol . At 29∘C , the rate constant is 0.0180s−1. At what temperature in degrees Celsius would this reaction go twice as fast? Solve the following equation for T2: ln ⁡(k2/k1) = Ea/R (1/T1−1/T2) The temperatures must be in kelvins and the activation energy must be in J/mol. Use the following value for the gas constant: R=8.314 J/mol⋅K.
Another first-order reaction also has a rate constant of 2.15×10−2s−1 at 25 ∘C. What is the value of k at 55 ∘C if E_2 = 130 kJ/mol ? Express your answer in reciprocal seconds to three significant figures.