A(g) + B(g) C(g) The rate law for the above reaction is: -d[A]/dt k[A][B] The rate constant is 2.75x101 L moll s1 at 3 Use the Arrhenius equation k = Ae Ea/RT to: Calculate Ea for this reaction. 31862.9J 0°C and 3.47x102 L moll s¹ at 512.0°C. Submit Answer You have entered that answer before Incompatible units. No conversion found between "a" and the required units. Calculate the rate constant k at 391.0°C for this reaction. Submit Answer Tries 0/15 Calculate the pre-exponential factor A for this reaction. Tries 0/15 Previous Tries
A(g) + B(g) C(g) The rate law for the above reaction is: -d[A]/dt k[A][B] The rate constant is 2.75x101 L moll s1 at 3 Use the Arrhenius equation k = Ae Ea/RT to: Calculate Ea for this reaction. 31862.9J 0°C and 3.47x102 L moll s¹ at 512.0°C. Submit Answer You have entered that answer before Incompatible units. No conversion found between "a" and the required units. Calculate the rate constant k at 391.0°C for this reaction. Submit Answer Tries 0/15 Calculate the pre-exponential factor A for this reaction. Tries 0/15 Previous Tries
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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![Arrhenius Equation
A(g) + B(g) → C(g)
The rate law for the above reaction is:
-d[A]/dt k[A][B]
The rate constant is 2.75×101 L mol1 s1 at 311.0°C and 3.47x102 L mol¹ 5¹ at 512.0°C.
Use the Arrhenius equation
k= Ae Ea/RT
to:
Calculate Ea for this reaction.
31862.9J
Submit Answer You have entered that answer before Incompatible units. No conversion found between "a" and the required units.
Calculate the rate constant k at 391.0°C for this reaction.
Submit Answer Tries 0/15
Calculate the pre-exponential factor A for this reaction.
Submit Answer Tries 0/15
Tries 0/15 Previous Tries](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3960258a-226b-4f65-b265-c9d5c73dd12c%2F658643ef-956c-4560-a173-f95b424a43f3%2Fyzadqn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Arrhenius Equation
A(g) + B(g) → C(g)
The rate law for the above reaction is:
-d[A]/dt k[A][B]
The rate constant is 2.75×101 L mol1 s1 at 311.0°C and 3.47x102 L mol¹ 5¹ at 512.0°C.
Use the Arrhenius equation
k= Ae Ea/RT
to:
Calculate Ea for this reaction.
31862.9J
Submit Answer You have entered that answer before Incompatible units. No conversion found between "a" and the required units.
Calculate the rate constant k at 391.0°C for this reaction.
Submit Answer Tries 0/15
Calculate the pre-exponential factor A for this reaction.
Submit Answer Tries 0/15
Tries 0/15 Previous Tries
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