How many grams of NO2 are needed to form 100.0g of HNO3?
Step 1) How do you get from NO2 to HNO3? What are your reactants? Write a reaction and balance your equation.
4NO2+2H2O+O2 --> 4HNO3
Step 2) Look at the stoichiometric ratio of the reaction.
100 g of HNO3 x (1 mol of HNO3/63.01 g) x (4mol NO2/4molHNO3)x (46.00 g NO2 /mol NO2) = 73 g
To determine the number of grams of NO2 needed to form 100.0g of HNO3, we need to use the balanced chemical equation. Let's start by writing the balanced equation for the reaction:
2 NO2 + H2O → HNO3 + HNO2
From the balanced equation, we can see that 2 moles of NO2 are required to produce 1 mole of HNO3.
Now, we need to convert the mass of HNO3 into moles. To do this, we divide the given mass of HNO3 (100.0g) by its molar mass. The molar mass of HNO3 is calculated by adding the atomic masses of hydrogen (H), nitrogen (N), and oxygen (O) in the compound:
HNO3: (1 x 1.01g/mol) + (1 x 14.01g/mol) + (3 x 16.00g/mol) = 63.02g/mol
Moles of HNO3 = Mass of HNO3 / Molar mass of HNO3
= 100.0g / 63.02g/mol
≈ 1.586 mol
Since the stoichiometric ratio between NO2 and HNO3 is 2:1, we need double the number of moles of NO2 compared to moles of HNO3.
Moles of NO2 = 2 x Moles of HNO3
= 2 x 1.586 mol
≈ 3.172 mol
Finally, we convert moles of NO2 to grams by multiplying the moles by the molar mass of NO2. The molar mass of NO2 is calculated by adding the atomic masses of nitrogen (N) and oxygen (O) in the compound:
NO2: (1 x 14.01g/mol) + (2 x 16.00g/mol) = 46.01g/mol
Grams of NO2 = Moles of NO2 x Molar mass of NO2
= 3.172 mol x 46.01g/mol
≈ 146.0g
Therefore, approximately 146.0 grams of NO2 are needed to form 100.0 grams of HNO3.