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 answers to the questions: i) Avogadro number The Avogadro number is the number of constituent particles (atoms, molecules, ions, or other particles) that are contained in one mole of a substance. It is defined as the number of atoms in exactly 12 grams of the carbon-12 isotope. Its approximate value is 6.022 × 10^23 mol^-1. ii) Determine the value of n in CuSO_4 · nH_2O. Given: Mass of hydrated copper(II) sulfate (CuSO_4 · nH_2O) = 7.50 g Mass of anhydrous copper(II) sulfate (CuSO_4) = 4.80 g Step 1: Calculate the mass of water of crystallization. The mass of water lost upon heating is the difference between the mass of the hydrated salt and the anhydrous salt. Mass of H_2O = Mass of hydrated CuSO_4 - Mass of anhydrous CuSO_4 Mass of H_2O = 7.50 g - 4.80 g = 2.70 g Step 2: Calculate the moles of anhydrous copper(II) sulfate. First, determine the molar mass of CuSO_4. (Atomic masses: Cu = 63.5, S = 32.1, O = 16.0) Molar mass of CuSO_4 = 63.5 + 32.1 + (4 × 16.0) = 63.5 + 32.1 + 64.0 = 159.6 g/mol Now, calculate the moles of CuSO_4. Moles of CuSO_4 = Mass of CuSO_4Molar mass of CuSO_4 = 4.80 g159.6 g/mol ≈ 0.030075 mol Step 3: Calculate the moles of water. First, determine the molar mass of H_2O. (Atomic masses: H = 1.0, O = 16.0) Molar mass of H_2O = (2 × 1.0) + 16.0 = 18.0 g/mol Now, calculate the moles of H_2O. Moles of H_2O = Mass of H_2OMolar mass of H_2O = 2.70 g18.0 g/mol = 0.15 mol Step 4: Determine the mole ratio to find n. The value of n is the ratio of moles of water to moles of anhydrous copper(II) sulfate. n = Moles of H_2OMoles of CuSO_4 = 0.15 mol0.030075 mol ≈ 4.987 Rounding to the nearest whole number, n = 5. The value of n is 5. Drop the next question.