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
- Mata NLv 410 years agoFavorite 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.