Question

nitrogen dioxide gas reacts with water to form nitric acid and nitrogen monoxide gas. if 50.0g NO2 and 5.00g h2o are mixed how many grams of excess reagent remain?

Answer 1

Balanced equation:
3 NO₂ + H₂O ===> 2 HNO₃ + NO
Reaction type: double replacement

50.0g NO2 = 50 / 46 =  1.086 Moles

5.00g h2o = 5 / 18 =  0.277 Moles

NO2 present is excess and Limiting reagent is water

Moles of water reacted = 0.277

Moles of NO2 reacted = 0.277 x 3 =  0.8326 Moles

Mass of NO2 reacted = 0.8326 x 46 =  38.30

Excess of NO2 present after reaction = 50 - 38.3 = 11.7 gm