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In the gas phase, carbon can react with oxygen in two different ways as shown b…

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Wize University Chemistry Textbook > Kinetics

Arrhenius Equation

4 Activities

In the gas phase, carbon can react with oxygen in two different ways as shown below.
C+O2→k1CO2Ea=24.6kJ/molC+O_2 \xrightarrow{k_1} CO_2 \hspace{20pt} E_a=24.6kJ/mol
C+0.5O2→k2COEa=19.6kJ/molC+0.5O_2 \xrightarrow{k_2} CO \hspace{20pt} E_a=19.6kJ/mol
At room temperature the amount of CO and CO2 produced are approximately equal. At what temperature would the reaction produce a 10:1 ratio of CO to CO2?
[Do NOT include units in your answers]
More Arrhenius Equation Questions:
Kinetics: Arrhenius Equation
What is the activation energy of a reaction if the rate constant at 40oC is double the value of the rate constant at 25oC?
A Schiff base reaction between 3-propanone and aniline proceeds with rate constants of 0.0065 M-1 s -1 and 0.0084 M-1 s -1 at 30oC and 80oC respectively. Determine the activation energy for this reaction.
Report your answer in kJ/mol to two decimal places.
In the gas phase, carbon can react with oxygen as shown below.
C+O2→k1CO2Ea=24.6 kJ/mol\rm C\quad+\quad O_2\quad\overset{k_1}{\overrightarrow{\hspace{1.5cm}}}\quad CO_2\qquad E_a=24.6\ kJ/mol
a) If the reaction is run at room temperature the rate constant is found to be 0.04 atm s−10.04\ atm\ s^{-1}. Determine the pre-exponential factor AA.
A first order gas phase reaction N2O4 → 2 NO2 was carried out isothermally and the activation barrier was found to be 23.5 kJ/mol. Initially p(N2O4) = 2.6 atm and p(NO2) = 0. After 1 hour p(NO2) = 2.0 atm and p(N2O4) =1.6 atm. Assume that both NO2 and N2O4 are ideal gases.
Determine the first order rate constant k, and the half life t1/2.
The above reaction was performed at 220oC. Calculate the pre-exponential factor.
Kinetics: Arrhenius Equation
What is the activation energy of a reaction if the rate constant at 40oC is double the value of the rate constant at 25oC?