Question

2
Nitric acid is manufactured by the Ostwald process, in which nitrogen dioxide reacts with water.
3 NO, (g) + H,O (1) ► 2 HNO, (aq) + NO (8)
How many grams of nitrogen dioxide are required in this reaction to produce 25.2 gm HNO, ?
​

Answer 1

Answer: 27.6 grams

Explanation:

$3NO_2+H_2O\rightarrow 2HNO_3+NO$

According to avogadro's law, 1 mole of every substance occupies 22.4 Liters at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

According to stochiometry,

2 moles of $HNO_3$ are produced by 3 moles of $NO_2$

$2\times 63=126 g$ of  $HNO_3$ is produced by =$3\times 46=138 g$ of $NO_2$

Thus 25.2 g of  $HNO_3$ is produced by =$\frac{138}{126}\times 25.2=27.6g$ of $NO_2$

Answer 2

The equation for this step of the process should be as follows, providing us with the molar ratio of HNO3 to NO2:

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

We also need the molecular mass of NO2 (46.0066g/mol) and HNO3 (63.01g/mol).

Using the mass of HNO3, 25.2 g would be equivalent to 25.2g(1mol/63.01g)= 0.399937 mol of HNO3.

Based on the molar ratio of HNO3 to NO2 (2 mol HNO3 to 3 mol NO2), the reaction would require 0.399937mol(3mol/2mol)= 0.599905 mol of NO2.

Using the mass of NO2, we would require 0.599905mol(46.0055g/1mol)= 27.6 g

If you like this don't forget to thank me and mark me as BRAINIEST