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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You're asking about Step 2 in Problem 1, part b, which determines the factor 'n' to find the molecular formula. Here's a detailed explanation: Empirical Formula: This is the simplest whole-number ratio of atoms in a compound. For example, if a compound has 2 carbons and 4 hydrogens, its empirical formula is CH_2. Molecular Formula: This is the actual number of atoms of each element in a molecule of the compound. For the example above, if the actual molecule has 4 carbons and 8 hydrogens, its molecular formula is C_4H_8. Notice that C_4H_8 is (CH_2)_4. The molecular formula is always a whole-number multiple of the empirical formula. This whole number is what we call 'n'. Molecular Formula = (Empirical Formula)_n To find 'n', we use the masses: n = Molecular massEmpirical formula mass In Problem 1: 1. We found the empirical formula in part (a) to be CH_2. 2. We calculated the empirical formula mass of CH_2: (1 × 12) + (2 × 1) = 14 g/mol. 3. The problem statement gives the molecular mass as 70 g/mol. So, to find 'n': n = 70 g/mol14 g/mol = 5 This means the actual molecule is 5 times larger than the empirical formula unit. Therefore, the molecular formula is (CH_2)_5, which simplifies to C_5H_10. That's 2 down. 3 left today — send the next one.