Final answer:
The empirical formula is determined by finding the simplest whole-number ratio of moles of each element in the compound. The provided molar ratios of C:N and H:N do not adequately correspond to the whole numbers needed for the empirical formula C5H7N as mentioned in the reference. There seems to be an error as per the given molar amounts and the stated empirical formula and its mass.
Step-by-step explanation:
The empirical formula for a compound is the simplest whole-number ratio of atoms in the compound. To find the empirical formula for a compound composed of 0.1470 mol C, 0.0735 mol H, and 0.0367 mol N, we first calculate the molar ratios of these elements to the element with the smallest number of moles, which is nitrogen (N) in this case.
The C-to-N molar ratio is 0.1470 mol C / 0.0367 mol N, which simplifies approximately to 4, indicating there are 4 times as many carbon atoms as nitrogen atoms. Similarly, the H-to-N molar ratio is 0.0735 mol H / 0.0367 mol N, which simplifies approximately to 2, indicating there are 2 times as many hydrogen atoms as nitrogen atoms. Therefore, these ratios are not adequately close to whole numbers.
To correct this, we must find a common multiple that can bring these ratios closer to whole numbers. If we multiply each ratio by 2, we get approximately C8 and H4 for every N. Thus, the empirical formula becomes C4H2N. However, there is a discrepancy in the example provided which indicates the empirical formula is C5H7N with an empirical formula mass of 81.13 g/mol. It seems there may be an error in the information given as the ratios calculated do not correspond to this empirical formula.