Chemistry, asked by venuchaitanya7777, 6 months ago

Nitric acid is manufactured by the ostwald process, in which nitrogen dioxide reacts with water. 3NO2 +H2O - 2HNO3 + NO. How many grams of nitrogen dioxide are required in this reaction to produce 25.2g HNO3 ?

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Answered by kolarykuttan
2

Answer:

Nitric acid is manufactured by the Ostwald process, in which nitrogen oxide reacts with water. How many grams of nitrogen dioxide are required in this reaction to produce 25.2 g of HNO3?

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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

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