Question

How many grams of NO2 are needed to form 88.0 g of HNO3?

Answer 1

64.4g

Step-by-step explanation:

The chemical reaction that will produce HNO₃ from NO₂ is given below:

3NO₂ + H₂O → 2HNO₃ + NO

Given;

Mass of HNO₃ = 88g

Now;

To solve this problem, find the number of moles of HNO₃;

Number of moles =
`(mass)/(molar mass)`

Molar mass of HNO₃ = 1 + 14 + 3(16) = 63g/mol

Number of moles =
`(88)/(63)` = 1.40mol

From the balanced reaction;

2 mole of HNO₃ is produced from 3 mole of NO₂

1.4 mole of HNO₃ will be produced from
`\frac{1.4 x 3} {2}` = 2.1mole of NO₂

Mass of NO₂ = number of moles x molar mass

Molar mass of NO₂ = 14 + 2(16) = 46g/mol

Mass of NO₂ = 1.4 x 46 = 64.4g