Chemistry
posted by Krissy .
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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!

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/t_{1/2}
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.