Question

How many grams of HNO3 are produced when 60.0 g of NO2 completely reacts?

Answer 1

Answer:

54.756 g

Explanation:

Assuming the equation for the reaction in question;

3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g)

We are given;

• Mass of NO₂ as 60.0 g

We are required to calculate the mass of HNO₃ produced

• We can calculate the mass of HNO₃ produced using the following simple steps;

Step 1: Calculate the moles of NO₂

Moles = Mass ÷ Molar mass

Molar mass of NO₂ = 46.01 g/mol

Therefore;

Moles of NO₂ = 60.0 g ÷ 46.01 g/mol

                       = 1.304 moles

Step 2: Calculate the moles of HNO₃ produced

From the equation, 3 moles of NO₂ reacted to produce 2 mole of HNO₃

Therefore, the mole ratio of NO₂ to HNO₃ is 3 : 2

Thus;

Moles of HNO₃ = Moles of NO₂ × 2/3

                          = 1.304 moles × 2/3

                          = 0.869 Moles

Step 3: Calculate the mass of HNO₃

Mass = Moles × Molar mass

Molar mass of HNO₃ = 63.01 g/mol

Therefore;

Mass = 0.869 moles × 63.01 g/mol

         = 54.756 g

Thus, the mass of HNO₃ produced is 54.756 g