General Chemistry

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NH4+ + NO2- = N2 + 2H2O
A reaction is run, and the liberated N2 gas is collected in a previously evacuated 500 mL container. After the reaction has gone on for 750 seconds, the pressure of N2 in the 500 mL container is 2.77 x 10^-2 atm , and the temperature of the N2 is 250 degrees celsius. Calculate the number of moles of N2 liberated and then calculate the average rate of the reaction

  • General Chemistry -

    Please show steps! Thanks!

  • General Chemistry -

    You should be able to ue PV = nRT and solve for n. Essy enough.

    Then rate is= delta(N2)/delta Time)
    Remember for (N2), that is mols/L. You will have mols and L.

  • General Chemistry -

    That's the equation I used! I found moles to be
    3.22 x 10^-4 mol and concentration to be 6.45 x 10^-4 M.
    I found the rate to be 8.60 x 10^-7 M/s, but the answer in my textbook is 7.55 x 10^-7 M/s

  • General Chemistry -

    So I am not sure where things are going wrong?

  • General Chemistry -

    Except for some rounding differences I get the same thing. I get 3.23E-4 mols

  • General Chemistry -

    Was the concentration of 6.45 x 10^-4 M correct? Just so I know I understand the concept?

  • General Chemistry -

    I obtained that number also.

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