Anonymous
Anonymous asked in Science & MathematicsEngineering · 10 years ago

Help! Please please answer this chemistry question below?

Consider the oxidation of nitric acid t nitrogen dioxide: 2NO (g) + O2 (g) → 2NO2 (g)

100.0 mL of NO at STP is mixed with 400.0 mL of O2 at STP. Afte the reaction goes to completion, what is the partial pressure of NO2 in the reaction mixture if the total pressure is 1 atm? PLEASE GIVE ME UR COMPLETE SOLUTION & NOT JUST THE FINAL ANSWER BECAUSE I REALLY DON'T KNOW HOW TO SOLVE THIS ONE.

a) 0.222 atm

b) 0.333 atm

c) 0.286 atm

d) 0.250 atm

e) 1.00 atm

1 Answer

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  • Mata N
    Lv 4
    10 years ago
    Favorite Answer

    From the reaction equation 100 mL of NO require 1/2 x 100 mL of O2 to react completely to NO2.

    Before the reaction:

    100 mL of NO + 0 mL of NO2 + 400 mL of NO

    After the reaction

    0 mL of NO + 100 mL of NO2 + (400 -100 x 1/2) = 350 mL of O2

    Total volume after reaction = 100 + 350 = 450 mL

    Partial pressure of NO2 = Volume of NO2/(Total Volume of Gas) x Total pressure

    = 100/350 x 1 atm = 0,286 atm

    Answer c) is the correct one.

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