Part A The Arrhenius equation shows the relationship between the rate constant k and the temperature T in kelvins and is typically written as k = Ae E/RT where Ris the gas constant (8.314 J/mol - K), A is a constant called the frequency factor, and E, is the activation energy for the reaction. The activation energy of a certain reaction is 36.3 kJ/mol. At 22 °C, the rate constant is 0.0180s. At what temperature in degrees Celsius would this reaction go twice as t Express your answer with the appropriate units. However, a more practical form of this equation is In 3(뉴 ) T = Value Units which is mathmatically equivalent to where ki and kz are the rate constants for a single reaction at two different absolute temperatures (T and T2). Part B Given that the initial rate constant is 0.0180s at an initial temperature of 22 °C, what would the rate constant be at a temperature of 140. °C for the same reaction described Express your answer with the appropriate units. kz = Value Units Submit Request Answer
Part A The Arrhenius equation shows the relationship between the rate constant k and the temperature T in kelvins and is typically written as k = Ae E/RT where Ris the gas constant (8.314 J/mol - K), A is a constant called the frequency factor, and E, is the activation energy for the reaction. The activation energy of a certain reaction is 36.3 kJ/mol. At 22 °C, the rate constant is 0.0180s. At what temperature in degrees Celsius would this reaction go twice as t Express your answer with the appropriate units. However, a more practical form of this equation is In 3(뉴 ) T = Value Units which is mathmatically equivalent to where ki and kz are the rate constants for a single reaction at two different absolute temperatures (T and T2). Part B Given that the initial rate constant is 0.0180s at an initial temperature of 22 °C, what would the rate constant be at a temperature of 140. °C for the same reaction described Express your answer with the appropriate units. kz = Value Units Submit Request Answer
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter13: Chemical Kinetics
Section: Chapter Questions
Problem 13.23QE: Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure...
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please answer all as they are part of 1 question but different questions,,.
![Part A
The Arrhenius equation shows the relationship between the rate constant k and
the temperature T in kelvins and is typically written as
The activation energy of a certain reaction is 36.3 kJ/mol . At 22 °C , the rate constant is 0.0180s¬1 . At what temperature in degrees Celsius would this reaction go twice as fast?
k = Ae-Ea/RT
where R is the gas constant (8.314 J/mol · K), A is a constant called the
frequency factor, and Ea is the activation energy for the reaction.
Express your answer with the appropriate units.
However, a more practical form of this equation is
HA
?
In=( -)
k2
k1
Ea
1
1
R
T
T,
which is mathmatically equivalent to
T, =
Value
Units
k1
E.
In
k2
T
T
R
where ki and k2 are the rate constants for a single reaction at two different
absolute temperatures (T1 and T2 ).
Part B
Given that the initial rate constant is 0.0180s- at an initial temperature of 22 °C, what would the rate constant be at a temperature of 140. °C for the same reaction described in Part A?
Express your answer with the appropriate units.
?
k2 =
Value
Units
Submit
Request Answer](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8b344f2f-3e6c-4999-84b7-e2733d707f50%2Fe7e1ab6f-0d2c-4d07-b135-c5e48973d1b7%2Fv8ssbwq_processed.png&w=3840&q=75)
Transcribed Image Text:Part A
The Arrhenius equation shows the relationship between the rate constant k and
the temperature T in kelvins and is typically written as
The activation energy of a certain reaction is 36.3 kJ/mol . At 22 °C , the rate constant is 0.0180s¬1 . At what temperature in degrees Celsius would this reaction go twice as fast?
k = Ae-Ea/RT
where R is the gas constant (8.314 J/mol · K), A is a constant called the
frequency factor, and Ea is the activation energy for the reaction.
Express your answer with the appropriate units.
However, a more practical form of this equation is
HA
?
In=( -)
k2
k1
Ea
1
1
R
T
T,
which is mathmatically equivalent to
T, =
Value
Units
k1
E.
In
k2
T
T
R
where ki and k2 are the rate constants for a single reaction at two different
absolute temperatures (T1 and T2 ).
Part B
Given that the initial rate constant is 0.0180s- at an initial temperature of 22 °C, what would the rate constant be at a temperature of 140. °C for the same reaction described in Part A?
Express your answer with the appropriate units.
?
k2 =
Value
Units
Submit
Request Answer
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