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OpenStudy (anonymous):
dinitrogen pentoxide decomposes in chloroform at a rate of 2.48 X 10^-4 mol/(L.min) at a particular temperature according to the equation 2N2O5-->4NO2+O2. The reaction is first order in N2O5. Given an initial concentration 0.400 mol/L, what is the rate constant for the reaction? What is the approximate (N2O5) after the reaction proceeds for 1.30h?
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OpenStudy (anonymous):
@abb0t
OpenStudy (aaronq):
you can use the integrated form the first order rate law: \(ln [A] = -kt + ln [A_o]\)
OpenStudy (anonymous):
What do the letters stand for?
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