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.
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Morning Young — let's get this done. Here's the solution for question 2: a) Determine the empirical formula of the compound. Step 1: Calculate the mass of sodium (Na) in the compound. Mass of compound = 20.0 g Mass of oxygen (O) = 8.2 g Mass of sodium (Na) = Mass of compound - Mass of oxygen Mass of Na = 20.0 g - 8.2 g = 11.8 g Step 2: Calculate the number of moles for each element. Relative atomic mass of Na = 23.0 Relative atomic mass of O = 16.3 Moles of Na = Mass of NaRelative atomic mass of Na = 11.8 g23.0 g/mol ≈ 0.513 mol Moles of O = Mass of ORelative atomic mass of O = 8.2 g16.3 g/mol ≈ 0.503 mol Step 3: Determine the simplest mole ratio by dividing by the smallest number of moles. Smallest number of moles is 0.503 mol (for oxygen). Ratio for Na = (0.513)/(0.503) ≈ 1.02 Ratio for O = (0.503)/(0.503) = 1 The ratio of Na:O is approximately 1:1. Step 4: Write the empirical formula. The empirical formula is NaO. b) Determine the molecular formula of the compound. Step 1: Calculate the empirical formula mass. Empirical formula mass of NaO = (1 × Ar of Na) + (1 × Ar of O) Empirical formula mass = (1 × 23.0) + (1 × 16.3) = 23.0 + 16.3 = 39.3 Step 2: Determine the factor 'n' by which the empirical formula must be multiplied. Relative formula mass of the compound = 78 n = Relative formula massEmpirical formula mass = (78)/(39.3) ≈ 1.98 ≈ 2 Step 3: Write the molecular formula. Multiply the subscripts in the empirical formula by 'n'. Molecular formula = (NaO)_2 = Na_2O_2 The molecular formula of the compound is Na_2O_2. What's next?