How many grams of 68% nitric acid do you need to take to get 27.6 g of nitric oxide (IV)?

We compose the reaction equation.
4NO2 + O2 + 2H2O = 4HNO3;
Find the molar mass of nitric oxide.
M (NO2) = NO2 – 46 g / mol;
Find the molar mass of nitric acid.
M (HNO3) = 63 g / mol.
Next, we make up the proportion.

27.6 g – x g;
4 × 46 g / mol – 4 × 63 g / mol.
Find the unknown x.

x = 27.6 g × 4 × 63 g / mol / 4 × 46 g / mol = 6955, 2 ÷ 184 = 37.8 g of nitric acid.

Next, we make up the proportion.
37.8 g – 68% HNO3;
x g – 100%.
Find the unknown value of x.
x = 37.8 × 100 ÷ 68 = 55.6 g.
That is, you need to take 55.6 grams of nitric acid.
Answer: m (HNO3) = 55.6 g.