How many grams of NO2 are needed to form 86.0 g of HNO3

Answer 1

3NO₂ (g) + H₂O(l) → 2HNO₃ (aq) + NO(aq)

molar mass of HNO₃ = 53g/mol

molar mass of NO₂ = 46 g/mol

mass of HNO₃ formed = 86.0g

In this balanced reaction for every 3 moles of nitrous oxide we create 2 moles of nitric acid. Using this we can convert from moles of nitric acid to moles of nitrous oxide like so:

86.0g / 53 gmol HNO₃ x (3 moles NO₂ / 2 moles HNO₃ ) x 46 gmol NO₂ = 112.0g of NO₂ needed to produce 86 grams of HNO₃

Hope this helps!