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.<br /><br />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:<br /><br />Mass of nitrogen = Total mass of compound - Mass of oxygen<br />Mass of nitrogen = 8.8g - 3.2g<br />Mass of nitrogen = 5.6g<br /><br />Next, 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:<br /><br />Moles of nitrogen = Mass of nitrogen / Atomic mass of nitrogen<br />Moles of nitrogen = 5.6g / 14.01g/mol<br />Moles of nitrogen ≈ 0.4 mol<br /><br />Moles of oxygen = Mass of oxygen / Atomic mass of oxygen<br />Moles of oxygen = 3.2g / 16.00g/mol<br />Moles of oxygen ≈ 0.2 mol<br /><br />Now, we need to find the ratio of moles of nitrogen to moles of oxygen:<br /><br />Ratio of nitrogen to oxygen = Moles of nitrogen / Moles of oxygen<br />Ratio of nitrogen to oxygen = 0.4 mol / 0.2 mol<br />Ratio of nitrogen to oxygen = 2<br /><br />Therefore, the empirical formula of the compound is $N_{2}O$.<br /><br />So, the correct answer is B. $N_{2}O$.