This physics problem tests your understanding of fundamental physical laws and their applications. The step-by-step solution below breaks down the problem using relevant equations and physical reasoning.
ScanSolve AI Answer
Step 1: Determine the percentage of oxygen. The sum of percentages of all elements in a compound must be 100%. Percentage of Oxygen = 100\% - (Percentage of Carbon + Percentage of Hydrogen) Percentage of Oxygen = 100\% - (52.17\% + 13\%) Percentage of Oxygen = 100\% - 65.17\% Percentage of Oxygen = 34.83\% Step 2: Assume a 100 g sample and convert percentages to masses. In a 100 g sample: Mass of Carbon (C) = 52.17 g Mass of Hydrogen (H) = 13 g Mass of Oxygen (O) = 34.83 g Step 3: Convert masses to moles using atomic masses. Atomic masses: C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol. Moles of Carbon: Moles of C = 52.17 g12.01 g/mol ≈ 4.344 mol Moles of Hydrogen: Moles of H = 13 g1.008 g/mol ≈ 12.897 mol Moles of Oxygen: Moles of O = 34.83 g16.00 g/mol ≈ 2.177 mol Step 4: Determine the simplest whole-number ratio by dividing by the smallest number of moles. The smallest number of moles is 2.177 mol (for Oxygen). Ratio for Carbon: 4.344 mol2.177 mol ≈ 1.995 ≈ 2 Ratio for Hydrogen: 12.897 mol2.177 mol ≈ 5.924 ≈ 6 Ratio for Oxygen: 2.177 mol2.177 mol = 1 The simplest whole-number ratio of C:H:O is 2:6:1. The empirical formula is C_2H_6O.