The following reaction is first order and the rate constant is 2.35 x 10^-4 s^-1 at 20 degress C.
2 N2O5 -----> 2 N2O4 + O2
A.) What is the rate of reaction if the [N2O5]=.25 M?
rate = k[N2O5]
B. What would the [N2O5] be after 100 s given that the initial [N2O5] was 0.25 M? What would be the [N2O4]
ln(Ao/A) = akt
C. What is the half life for this reaction?
k = 0.693/t1/2
D. How long will it take for the initial [N2O5]=0.88M to drop to 0.11 M?
ln(Ao/A) = akt
E) What is the activation energy for the reaction if the rate constant at 30 degrees C is 9.15 x 10^-4 s^-1
Use the Arrhenius equation.
F.) What is the rate constant at 70 degrees C?
Use the Arrhenius equation.
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Chemistry help needed... Confused?
The following reaction is first order and the rate constant is 2.35 x 10^-4 s^-1 at 20 degress C.
2 N2O5 -----> 2 N2O4 + O2
A.) What is the rate of reaction if the [N2O5]=.25 M?
B. What would the [N2O5] be after 100 s given that the initial [N2O5] was 0.25 M? What would be the [N2O4]
C. What is the half life for this reaction?
D. How long will it take for the initial [N2O5]=0.88M to drop to 0.11 M?
E) What is the activation energy for the reaction if the rate constant at 30 degrees C is 9.15 x 10^-4 s^-1
F.) What is the rate constant at 70 degrees C?
I'm confused on how to solve these and I have to show work. This is a sample problem for me to work on also all the C have to be changed by adding 273. If someone can show the work and how to get through this it would be very helpful! Thanks!
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