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Dinitrogen tetraoxide (N2O4) decomposes spontaneously at room temperature in the gas phase: N2O4(9) → 2NO2(g) The rate law governing the disappearance of N2O4 with time is d[N2O4] = k«[N2O4] dt At 30°C, k = 5.1 × 10® s-1 and the activation energy for the reaction is 54.0 kJ mol¬. (a) Calculate the time (in seconds) required for the partial pressure of N204(9) to decrease from 0.10 atm to 0.010 atm at 30°C. (b) Repeat the calculation of part (a) at 300°C.

Dinitrogen tetraoxide (N2O4) decomposes spontaneously at room temperature in the gas phase: N2O4(9) → 2NO2(g) The rate law governing the disappearance of N2O4 with time is d[N2O4] = k«[N2O4] dt At 30°C, k = 5.1 × 10® s-1 and the activation energy for the reaction is 54.0 kJ mol¬. (a) Calculate the time (in seconds) required for the partial pressure of N204(9) to decrease from 0.10 atm to 0.010 atm at 30°C. (b) Repeat the calculation of part (a) at 300°C.

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Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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38. Dinitrogen tetraoxide (N2O4) decomposes spontaneously at room temperature in the gas phase: N2O4(9) → 2NO2 (9) The rate law governing the disappearance of N2O4 with time is d[N2O4] k[N2O4] dt At 30°C, k = 5.1 × 106 s-1 and the activation energy for the reaction is 54.0 kJ mol¬1. (a) Calculate the time (in seconds) required for the partial pressure of N,04(g) to decrease from 0.10 atm to 0.010 atm at 30°C. (b) Repeat the calculation of part (a) at 300°C.
Transcribed Image Text:38. Dinitrogen tetraoxide (N2O4) decomposes spontaneously at room temperature in the gas phase: N2O4(9) → 2NO2 (9) The rate law governing the disappearance of N2O4 with time is d[N2O4] k[N2O4] dt At 30°C, k = 5.1 × 106 s-1 and the activation energy for the reaction is 54.0 kJ mol¬1. (a) Calculate the time (in seconds) required for the partial pressure of N,04(g) to decrease from 0.10 atm to 0.010 atm at 30°C. (b) Repeat the calculation of part (a) at 300°C.
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The given reaction is first order as governed by the rate law expression. The concentration of the reactant is raised to power one in the rate law expression.

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