{
  "id": "ca72b11c-e7da-54ed-a4f4-ede00baec661",
  "slug": "s1-4-counting-particles-by-mass-the-mole",
  "title": "S1.4 Counting particles by mass: The mole",
  "course": "IB Chemistry",
  "level": "SL",
  "syllabusCode": "S1.4",
  "questionCount": 14,
  "page": "https://splycr.com/ib-chemistry/s1-4-counting-particles-by-mass-the-mole",
  "data": "https://splycr.com/library/s1-4-counting-particles-by-mass-the-mole.json",
  "play": "https://splycr.com/?set=ca72b11c-e7da-54ed-a4f4-ede00baec661",
  "section": {
    "name": "Structure 1: Models of the particulate nature of matter",
    "page": "https://splycr.com/ib-chemistry/models-of-the-particulate-nature-of-matter"
  },
  "source": {
    "name": "Biology by Bradford",
    "href": "https://www.biologybybradford.com",
    "note": "Written for the splycr library by Biology by Bradford."
  },
  "questions": [
    {
      "number": 1,
      "question": "Number of particles in one mole of a substance?",
      "answer": "6.02 × 10²³",
      "wrongOptions": [
        "6.02 × 10²²",
        "3.01 × 10²³",
        "1.00 × 10²³"
      ]
    },
    {
      "number": 2,
      "question": "Mass of one mole of a substance, in g mol⁻¹?",
      "answer": "Molar mass",
      "wrongOptions": [
        "Relative atomic mass",
        "Molar volume",
        "Mass number"
      ]
    },
    {
      "number": 3,
      "question": "Weighted mean mass of an element's atoms compared with one-twelfth of a carbon-12 atom?",
      "answer": "Relative atomic mass",
      "wrongOptions": [
        "Molar mass",
        "Mass number",
        "Atomic number"
      ]
    },
    {
      "number": 4,
      "question": "Relative formula mass of H₂SO₄ (Ar: H 1, S 32, O 16)?",
      "answer": "98",
      "wrongOptions": [
        "97",
        "96",
        "50"
      ]
    },
    {
      "number": 5,
      "question": "Amount of water in 36 g of water (Mr = 18)?",
      "answer": "2.0 mol",
      "wrongOptions": [
        "0.50 mol",
        "36 mol",
        "1.0 mol"
      ]
    },
    {
      "number": 6,
      "question": "Mass of 0.25 mol of CaCO₃ (Mr = 100)?",
      "answer": "25 g",
      "wrongOptions": [
        "400 g",
        "2.5 g",
        "250 g"
      ]
    },
    {
      "number": 7,
      "question": "Number of oxygen atoms in 1 mol of CO₂?",
      "answer": "1.20 × 10²⁴",
      "wrongOptions": [
        "6.02 × 10²³",
        "1.81 × 10²⁴",
        "3.01 × 10²³"
      ]
    },
    {
      "number": 8,
      "question": "Empirical formula of C₆H₁₂O₆?",
      "answer": "CH₂O",
      "wrongOptions": [
        "C₂H₄O₂",
        "C₃H₆O₃",
        "CHO"
      ]
    },
    {
      "number": 9,
      "question": "A hydrocarbon has empirical formula CH₂ and Mr = 56. Its molecular formula?",
      "answer": "C₄H₈",
      "wrongOptions": [
        "C₂H₄",
        "C₃H₆",
        "C₅H₁₀"
      ]
    },
    {
      "number": 10,
      "question": "Percentage by mass of carbon in CH₄ (Mr = 16)?",
      "answer": "75%",
      "wrongOptions": [
        "25%",
        "20%",
        "80%"
      ]
    },
    {
      "number": 11,
      "question": "Concentration when 0.50 mol of NaCl makes 250 cm³ of solution?",
      "answer": "2.0 mol dm⁻³",
      "wrongOptions": [
        "0.125 mol dm⁻³",
        "0.50 mol dm⁻³",
        "4.0 mol dm⁻³"
      ]
    },
    {
      "number": 12,
      "question": "Amount of solute in 100 cm³ of 0.20 mol dm⁻³ solution?",
      "answer": "0.020 mol",
      "wrongOptions": [
        "20 mol",
        "0.20 mol",
        "2.0 mol"
      ]
    },
    {
      "number": 13,
      "question": "Volume of 1.0 mol dm⁻³ stock needed for 500 cm³ of 0.20 mol dm⁻³ solution?",
      "answer": "100 cm³",
      "wrongOptions": [
        "250 cm³",
        "2500 cm³",
        "40 cm³"
      ]
    },
    {
      "number": 14,
      "question": "Equal volumes of gases at the same temperature and pressure contain equal…?",
      "answer": "Numbers of particles",
      "wrongOptions": [
        "Masses",
        "Densities",
        "Numbers of atoms"
      ]
    }
  ]
}