Chemistry

dinitrogen pentoxide n2o5 decomposes by a first-order decomposition in chloroform solvent to yield NO2 and O2. The rate constant at 45°C is 6.2 x 10^-4 mins^-1. Calculate the volume of O2 obtained from the reaction of 1.00 mol N2O5 at 45°C and 770 mmHg after 20.0 hours.
N2O5 = 2 NO2 + 1/2 O2

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  1. Wouldn't this be
    ln(No/N) = kt
    You know No and k, t is given but change so k and t are in the same units. Solve for N = mols N2O5 at end of 20 hours, then take 1/2 that for mols O2 and use PV = nRT to calculate volume O2.

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    posted by DrBob222
  2. I keep getting 6.12 and the answer is suppose to be 6.8

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    posted by Veronica

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