Question: 1. The jars below, from left to right, each contain exactly one mole of carbon, sulfur, and aluminum, respectively. Which jar contains the most atoms? The jar of carbon. The jar of sulfur. The jar of aluminum. Each jar contains the same number of atoms. 2. If each jar below contains exactly one mole of each element, which jar contains the greatest mass? (The atomic mass of each element is given.) The jar of carbon. The jar of sulfur. The jar of aluminum. Each jar contains the same mass. 3. Note the mass of a copper(I) oxide formula unit in the image below. What is the mass of 8.250 moles of Cu₂O? 17.34 u 17.34 g 1,181 u 1,181 g 4. What is the mass of 8.12 × 10²³ molecules of CO₂ gas? (Atomic mass of carbon = 12.011 u; oxygen = 15.999 u.) 32.6 g 44.0 g 48.9 g 59.3 g 5. Sulfuric acid (H₂SO₄) has a molar mass of 98.1 g/mol. How many oxygen atoms are found in 75.0 g of H₂SO₄? 1.15 × 10²³ 1.84 × 10²⁴ 4.61 × 10²³ 7.87 × 10²³

1. **Problem:** Which jar contains the most atoms if each jar contains exactly one mole of carbon, sulfur, and aluminum? 2. **Problem:** Which jar contains the greatest mass if each jar contains exactly one mole of carbon (12.011 u), sulfur (32.065 u), and aluminum (26.982 u)? 3. **Problem:** What is the mass of 8.250 moles of Cu₂O if one formula unit has a mass of 143.091 u? 4. **Problem:** What is the mass of 8.12 \times 10^{23} molecules of CO₂ gas? (Atomic mass C = 12.011 u, O = 15.999 u) 5. **Problem:** How many oxygen atoms are in 75.0 g of H₂SO₄ (molar mass 98.1 g/mol)? --- ### Step 1: Number of atoms in each jar - One mole contains Avogadro's number of particles: $$6.022 \times 10^{23}$$ atoms. - Each jar contains exactly one mole of an element. - Therefore, **each jar contains the same number of atoms**. ### Step 2: Greatest mass among jars - Mass of 1 mole = atomic mass in grams. - Carbon: $$12.011\,g$$ - Sulfur: $$32.065\,g$$ - Aluminum: $$26.982\,g$$ - Sulfur has the greatest atomic mass, so the jar of sulfur has the greatest mass. ### Step 3: Mass of 8.250 moles of Cu₂O - Mass of 1 mole Cu₂O = $$143.091\,g$$ (given) - Mass of 8.250 moles = $$8.250 \times 143.091 = 1180.5\,g$$ - Rounded to 3 significant figures: $$1,181\,g$$ ### Step 4: Mass of 8.12 \times 10^{23} molecules of CO₂ - Molar mass CO₂ = $$12.011 + 2 \times 15.999 = 44.009\,g/mol$$ - Number of molecules given: $$8.12 \times 10^{23}$$ - Number of moles = $$\frac{8.12 \times 10^{23}}{6.022 \times 10^{23}} = 1.348\,mol$$ - Mass = $$1.348 \times 44.009 = 59.3\,g$$ ### Step 5: Number of oxygen atoms in 75.0 g of H₂SO₄ - Molar mass H₂SO₄ = $$98.1\,g/mol$$ - Moles of H₂SO₄ = $$\frac{75.0}{98.1} = 0.7645\,mol$$ - Each mole of H₂SO₄ contains 4 moles of oxygen atoms. - Moles of oxygen atoms = $$0.7645 \times 4 = 3.058\,mol$$ - Number of oxygen atoms = $$3.058 \times 6.022 \times 10^{23} = 1.84 \times 10^{24}$$ atoms --- **Final answers:** 1. Each jar contains the same number of atoms. 2. The jar of sulfur contains the greatest mass. 3. Mass of 8.250 moles of Cu₂O is $$1,181\,g$$. 4. Mass of $$8.12 \times 10^{23}$$ molecules of CO₂ is $$59.3\,g$$. 5. Number of oxygen atoms in 75.0 g of H₂SO₄ is $$1.84 \times 10^{24}$$ atoms.