The reaction between nitrogen dioxide and water to produce nitric acid can be represented by the following balanced chemical equation:

NO2 + H2O → HNO3



The molar mass of HNO3 can be calculated by adding the atomic masses of its constituent atoms, which are as follows:

H = 1.01 g/mol
N = 14.01 g/mol
O = 16.00 g/mol

Therefore, molar mass of HNO3 = 1.01 + 14.01 + (3 x 16.00) = 63.01 g/mol



Number of moles of HNO3 can be calculated by dividing the given mass of HNO3 (6.3 g) by its molar mass (63.01 g/mol):

Number of moles of HNO3 = 6.3 g / 63.01 g/mol = 0.1 mol



From the balanced chemical equation, we can see that 1 mole of NO2 reacts with 1 mole of HNO3. Therefore, the number of moles of NO2 required to produce 0.1 mol of HNO3 is also 0.1 mol.



The molar mass of NO2 can be calculated by adding the atomic masses of its constituent atoms, which are as follows:

N = 14.01 g/mol
O = 16.00 g/mol (2 atoms)

Therefore, molar mass of NO2 = 14.01 + (2 x 16.00) = 46.01 g/mol

Mass of NO2 required can be calculated by multiplying the number of moles of NO2 (0.1 mol) with its molar mass (46.01 g/mol):

Mass of NO2 = 0.1 mol x 46.01 g/mol = 4.601 g

Therefore, 4.601 g of nitrogen oxide is required to produce 6.3 g of HNO3.