Final answer:
To form 45.4 g of HNO3, approximately 33.12 g of nitrogen dioxide (NO2) are required.
Step-by-step explanation:
To determine the number of grams of nitrogen dioxide (NO2) required to form 45.4 g of HNO3, you need to balance the chemical equation for the reaction between nitrogen dioxide and water. The balanced equation is:
NO2 + H2O → HNO3
In this equation, the molar ratio between NO2 and HNO3 is 1:1. Therefore, the number of moles of NO2 required can be calculated by dividing the mass of HNO3 by its molar mass:
Number of moles of HNO3 = 45.4 g / molar mass of HNO3
Since the molar mass of HNO3 is approximately 63 g/mol, we can calculate the number of moles of NO2:
Number of moles of NO2 = 45.4 g / 63 g/mol = 0.72 mol
Finally, we can calculate the mass of NO2 using its molar mass:
Mass of NO2 = 0.72 mol * molar mass of NO2
Since the molar mass of NO2 is approximately 46 g/mol, we can calculate the mass:
Mass of NO2 = 0.72 mol * 46 g/mol = 33.12 g