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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Here are the solutions to the problems: Question 17: A student works a problem and finds that a compound has 0.074 moles of carbon and 0.148 moles of oxygen. What is the empirical formula of the compound? Step 1: Write down the moles of each element. Moles of Carbon (C) = 0.074 mol Moles of Oxygen (O) = 0.148 mol Step 2: Divide by the smallest number of moles to find the mole ratio. For C: 0.074 mol0.074 mol = 1 For O: 0.148 mol0.074 mol = 2 Step 3: Write the empirical formula. The ratio of C:O is 1:2. The empirical formula is CO_2. Question 18: What is the empirical formula for a compound that is 18.7% Li, 16.3% C, and 65.0% O? Step 1: Assume a 100 g sample. Mass of Li = 18.7 g Mass of C = 16.3 g Mass of O = 65.0 g Step 2: Convert mass to moles using atomic masses (Li ≈ 6.94 g/mol, C ≈ 12.01 g/mol, O ≈ 16.00 g/mol). Moles of Li: 18.7 g6.94 g/mol ≈ 2.69 mol Moles of C: 16.3 g12.01 g/mol ≈ 1.36 mol Moles of O: 65.0 g16.00 g/mol ≈ 4.06 mol Step 3: Divide by the smallest number of moles (1.36 mol). For Li: (2.69)/(1.36) ≈ 1.98 ≈ 2 For C: (1.36)/(1.36) = 1 For O: (4.06)/(1.36) ≈ 2.98 ≈ 3 Step 4: Write the empirical formula. The ratio of Li:C:O is 2:1:3. The empirical formula is Li_2CO_3. Question 19: A 100.0-g sample of a compound is made up of 35.9 g of aluminum and 64.1 g of sulfur. The empirical formula of the compound is Step 1: Write down the mass of each element. Mass of Al = 35.9 g Mass of S = $