Register
He specific rate constant, k, for the following first-order reaction is 9.16 x 10-3 s -1 at 0.0°C. The activation energy of this reaction is 88.0 kJ/mol. Determine the value of k at 2.0°C. N2O5  NO2 +
86.0k views
0 votes
He specific rate constant, k, for the following first-order

reaction is 9.16 x 10-3
s
-1 at 0.0°C. The activation energy of
this reaction is 88.0 kJ/mol. Determine the value of k at
2.0°C.
N2O5  NO2 + NO3

User Michaeldel
by
5.8k points

1 Answer

6 votes
Hope this helps. Thanks
He specific rate constant, k, for the following first-order reaction is 9.16 x 10-3 s-example-1
User Pgilmon
by
6.3k points
Ask a Question
Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.

6.5m questions

8.6m answers

Other Questions

Some elements can have multiple molecular forms in the same physical state. these multiple forms are called a. isotopes. b. isotropes. c. allotropes. d. multi-tropes.
True or false: in the water cycle, water returns to Earth as condesation, usually in the form of rain or snow.
The original amount of a radioactive sample should be multiplied by which expression to calculate the amount of the sample that remains after n half-lives have passed? (1/2)xn (1/n)^2 (1/2)^n 1/(2n)
How many moles of ca(no32 are in 400 ml of a 0.80 m calcium nitrate solution?
How do the number of daylight hours affect temperature
Link Copied!