Question
Determine the empirical formulas for the compounds with the following percent composition: 28.5% iron, 48.6% oxygen, and 22.9% 2.9% sulfur Fe_(2)S_(3)O_(6) Fe_(2)S_(4)O_(8) Fe_(3)S_(3)O_(9) Fe_(2)S_(3)O_(12)
Solution
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(208 Votos)
Diana
Veterano · Tutor por 9 anos
Resposta
To determine the empirical formula for the compound with the given percent composition, we need to convert the percentages to grams and then to moles.Given:- 28.5% iron (Fe)- 48.6% oxygen (O)- 22.9% sulfur (S)Assume we have 100 grams of the compound. This means we have:- 28.5 grams of Fe- 48.6 grams of O- 22.9 grams of SNext, we convert the masses to moles using the molar masses of each element:- Molar mass of Fe = 55.85 g/mol- Molar mass of O = 16.00 g/mol- Molar mass of S = 32.07 g/molCalculate the moles of each element:- Moles of Fe = 28.5 g / 55.85 g/mol = 0.511 moles- Moles of O = 48.6 g / 16.00 g/mol = 3.0375 moles- Moles of S = 22.9 g / 32.07 g/mol = 0.714 molesNow, we need to find the simplest whole number ratio of the moles of each element. To do this, we divide each mole value by the smallest mole value among them:- Smallest mole value = 0.511 moles (Fe)Divide each mole value by 0.511:- Fe: 0.511 / 0.511 = 1- O: 3.0375 / 0.511 = 5.95 ≈ 6- S: 0.714 / 0.511 = 1.4 ≈ 1The ratio of Fe:O:S is approximately 1:6:1. Therefore, the empirical formula for the compound is FeO6S.Among the given options, the correct empirical formula is Fe2S3O6.