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,0,] = 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 a. 0.10 atm to 0.010 atm at 30°C. b. Calculate the value of the rate constant at 300K. c. Repeat the calculation for the reaction in a) at the new temperature (300K). d. Write an observation about how the rate of reaction changed upon increasing the temperature.
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,0,] = 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 a. 0.10 atm to 0.010 atm at 30°C. b. Calculate the value of the rate constant at 300K. c. Repeat the calculation for the reaction in a) at the new temperature (300K). d. Write an observation about how the rate of reaction changed upon increasing the temperature.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 12PS: The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table...
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how do i do b c and d
![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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc16206f4-19bf-423e-ba9e-756d199d055d%2F1d71d639-9f3b-4d58-82aa-0b839f703a28%2Fln6l2pg_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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.
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