Posted by **Krissy** on Tuesday, November 20, 2012 at 11:54am.

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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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