1) The activation energy for the following first-order reaction is 102 kJ/mol. N₂O5(g) → 2NO2(g) + (1/2)0₂(g) The value of the rate constant (k) is 1.35 x 10-4 s-¹ at 35°C. What is the value of k at 0°C? (R= 8.314 J/mol-K) A. 8.2 x 10-7 s-1 B. 1.9 x 10-5 S-1 C. 4.2 x 10-5 sS-1 D. 2.2 x 10-² S-1
1) The activation energy for the following first-order reaction is 102 kJ/mol. N₂O5(g) → 2NO2(g) + (1/2)0₂(g) The value of the rate constant (k) is 1.35 x 10-4 s-¹ at 35°C. What is the value of k at 0°C? (R= 8.314 J/mol-K) A. 8.2 x 10-7 s-1 B. 1.9 x 10-5 S-1 C. 4.2 x 10-5 sS-1 D. 2.2 x 10-² S-1
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 23PS: The decomposition of ammonia on a metal surface to form N2 and H2 is a zero-order reaction (Figure...
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Directions: Answer the following problems by showing the complete solution. In return, I will give you a good and high rating. Thank you so much!
Note: Please be careful with the units and measurements in calculations. Thank you!
No. 1-2.
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