39 - (CHEMUILHI Summer, 2022,03) - Stochiometric Relationship 8.8g of an oxide of nitrogen contains 3.2g of oxygen. What is the empirical formula of the compound? A. N_(2)O_(5) B. N_(2)O C. NO_(2) D. NO

To find the empirical formula of the compound, we need to determine the ratio of nitrogen to oxygen in the compound.First, let's find the mass of nitrogen in the compound. We can do this by subtracting the mass of oxygen from the total mass of the compound:Mass of nitrogen = Total mass of compound - Mass of oxygenMass of nitrogen = 8.8g - 3.2gMass of nitrogen = 5.6gNext, we need to convert the masses of nitrogen and oxygen to moles. We can do this by dividing the mass of each element by its respective atomic mass:Moles of nitrogen = Mass of nitrogen / Atomic mass of nitrogenMoles of nitrogen = 5.6g / 14.01g/molMoles of nitrogen ≈ 0.4 molMoles of oxygen = Mass of oxygen / Atomic mass of oxygenMoles of oxygen = 3.2g / 16.00g/molMoles of oxygen ≈ 0.2 molNow, we need to find the ratio of moles of nitrogen to moles of oxygen:Ratio of nitrogen to oxygen = Moles of nitrogen / Moles of oxygenRatio of nitrogen to oxygen = 0.4 mol / 0.2 molRatio of nitrogen to oxygen = 2Therefore, the empirical formula of the compound is .So, the correct answer is B. .