Its an old study set, and i have calculated question 1 and 2, but i cant seem to get my values right. So i would really appreciate some help with the calculations for the following: Nitrogen pentoxide decomposes according to the reaction:

N₂O5 -> NO₂ + NO2 + 1/2 O₂

The reaction is a first order reaction, and has a rate constant k.

T(K)	273	298	308	318	328	338
k(s -1)	7.87x10-7	3.46 x10-5	13.5 x10-5	49.8 x10-5	150 x10-5	487 x10-5

Nitrogen pentoxide is unstable and a dangerous oxidant. We wish to design a plug-flow reactor, where we optain 95% decompostion to NO2 and O_2. The reactor need to operate at atmosferic pressure and 338 K. the feed is pure pentoxide, and F_A0 = 1.0 mol/s.

question 1)

Make a stoichiometric table for the plug-flow reactor

question 2)

Find the volumetric gas flow (m3/s) in and out of the reactor, at the given temperature and pressure.

Determine the starting composition (mole fraction) from the reactor.

question 3)

How big of a reactor (m3) is nessesary to obtain the given degree of conversion (95%)?