Nitrogen and oxygen form an extensive series of oxides with the general formula N_xO_y.What is the empirical formula for an oxide that contains 30.44% by mass nitrogen?

Question

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To determine the empirical formula, we need the molar ratios of nitrogen and oxygen in the oxide. We know the oxide has 30.44% nitrogen, which means it must have 69.56% oxygen. We can assume a 100 g sample of the oxide, which means we have 30.44 g nitrogen and 69.56 g oxygen. Next, we need to find the mole ratio by dividing the mass by the molar mass: 30.44 g N / 14.01 g/mol = 2.17 mol N 69.56 g O / 16.00 g/mol = 4.35 mol O The simplest whole-number ratio of N to O is approximately 1:2, so the empirical formula is NO2. However, none of the answer choices match this formula exactly. We can see that choice C, NO₂, is closest to NO2, and it also includes the possibility of additional sulfur (which is present in some of the other oxides in the series). Therefore, the best choice is C.

Nitrogen and Oxygen Form an Extensive Series of Oxides with the General