This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
To determine the empirical formula, we first convert the given percentages to masses, then to moles, and finally find the simplest whole-number ratio of the moles. The question states: "An organic compound is composed of 62.17 Carbon, 10.41% hydrogen, and 27.8% Carbon, x oxygen." There appears to be a typo in the percentages. Based on the sum of percentages being close to 100% (62.17 + 10.41 + 27.8 = 100.38), we will assume the composition is: • Carbon (C): 62.17% • Hydrogen (H): 10.41% • Oxygen (O): 27.8% Step 1: Assume a 100 g sample. This converts the percentages directly into masses: Mass of C = 62.17 g Mass of H = 10.41 g Mass of O = 27.8 g Step 2: Convert the mass of each element to moles using their atomic masses (C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol). Moles of C: Moles of C = 62.17 g12.01 g/mol = 5.1765 mol Moles of H: Moles of H = 10.41 g1.008 g/mol = 10.3274 mol Moles of O: Moles of O = 27.8 g16.00 g/mol = 1.7375 mol Step 3: Divide each mole value by the smallest number of moles to find the simplest mole ratio. The smallest number of moles is 1.7375 mol (for Oxygen). Ratio for C: 5.1765 mol1.7375 mol ≈ 2.979 ≈ 3 Ratio for H: 10.3274 mol1.7375 mol ≈ 5.944 ≈ 6 Ratio for O: 1.7375 mol1.7375 mol = 1 Step 4: Write the empirical formula using these whole-number ratios. The empirical formula is C_3H_6O. The empirical formula of the compound is C_3H_6O. Send me the next one 📸