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)

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)

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

At 10oC and 50oC the first-order rate constants of a reaction are 9.88 x 10-4 and 9.45 x 10-2 s-1 respectively. What is the activation energy (kJ/mole)? (R = 8.31 J/mole oK). 87.2 78.2 27.8 28.7
18. * Determine the activation energy for the first-order reaction 2NOCI2NO + Cl2 given the following rate constants at different temperatures. Temperature (K) k (L/mol-s) 500 2.9 x 10-1 600 16.3 O 1.21 x 10* J/mol O 1.00 x 10s J/mol O 8.27 x 10 $ J/mol O 6.88 x 10-4 J/mol
The answer I have is wrong. It’s not to the 3rd or -3rd power.
5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 354.0 °C 3.9 x 10° 233.0 °C 1.5 x 10 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. a Round your answer to 2 significant digits. kJ E x10 a mol ?
A certain first order reaction has k = 2.51 s-1 . If the initial concentration of the reactant is 6.50 M, how much will be left after two half lives (in M)? Give your answer to three sig figs
3. You have a reaction that is run at 273°C and has a rate constant of 2.52 x 10/s. The same reaction is run at 157 °C and has a rate constant of 1.0 x 10-/s. What is the activation energy for this reaction? (R = 8.314 J/mol K) %3D 0.00898mols 102 sec 4. w for ate= k[NO2]?. The rate constant for this reaction: If yo tion for 5 minutes urd be the concentra
8. Dinitrogen tetraoxide (N2O4) decomposes spontaneously at room temperature in the gas phase: N2O4 (g) → 2 NO2(g) The rate law governing the disappearance of N2O4 with time is A[N,O4] = k N2O4]. At At 30°C, k = 5.1 x 106 s-1 and the activation energy for the reaction is 54.0 kJ/mol. Calculate the time (in seconds) required for the partial pressure of N2O4(g) to decrease from а. 0.10 atm to 0.010 atm at 30°C. b. Calculate the value of the rate constant at 300K. Repeat the calculation for the reaction in a) at the new temperature (300K). С. d. Write an observation about how the rate of reaction changed upon increasing the temperature.
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
10. The rate of a particular reaction increases from 0.10 M s¹ to 0.50 M s¹ when the temperature is increased from 25°C to 35°C. Calculate the activation energy for this reaction.
-1 For a certain reaction, the frequency factor A is 7.5 × 10⁹ s1 and the activation energy is 21.4 What is the rate constant for the reaction at 95. °C? Round your answer to 2 significant digits. Note: Reference the Fundamental constants table for additional information. k = -1 S X kJ mol S
The given first-order reaction A → B, has a rate constant of 1.60 x 10-2 s-1 at 165oC and 6.54 x 10-1 s-1 at 295oC. What is the activation energy for the reaction? 59.0 kJ/mol 650. kJ/mol 11.5 kJ/mol 0.582 kJ/mol