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Mole Concept and Avogadro's Law 🧮

Quiz by minna wahid

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30 questions
Show answers
  • Q1
    What is the number of units in 1 mole of any substance, according to Avogadro's constant (NA)?
    9.83 \times 10^{21}
    6.02 \times 10^{23}
    3.05 \times 10^{25}
    1.602 \times 10^{22}
    30s
  • Q2
    What is the volume of 1 mole of any gas at room temperature and pressure, according to Avogadro's Law?
    18 liters (L)
    30 liters (L)
    12 liters (L)
    24 liters (L)
    30s
  • Q3
    What is the formula to calculate the number of moles (n) when given the mass in grams (m) and the relative atomic or molecular mass (AR/MR) of a substance?
    Number of moles (n) = mass in grams (m) × relative atomic or molecular mass (AR/MR)
    Number of moles (n) = mass in grams (m) + relative atomic or molecular mass (AR/MR)
    Number of moles (n) = mass in grams (m) - relative atomic or molecular mass (AR/MR)
    Number of moles (n) = mass in grams (m) ÷ relative atomic or molecular mass (AR/MR)
    30s
  • Q4
    Calculate the volume of NH3 (ammonia) at room temperature and pressure given the mass of 28 grams. Use Rule 3 to find the volume of 1 mole of NH3 gas.
    0.75 liters (L)
    2.50 liters (L)
    1.17 liters (L)
    3.20 liters (L)
    30s
  • Q5
    Find the mass of 3 moles of H2O (water) molecules. Use Rule 2 to calculate the mass in grams of 3 moles of water.
    90 grams
    120 grams
    108 grams
    72 grams
    30s
  • Q6
    Calculate the mass of 2 moles of CO2 (carbon dioxide) molecules. Use Rule 2 to determine the mass in grams of 2 moles of carbon dioxide.
    66 grams
    96 grams
    88 grams
    72 grams
    30s
  • Q7
    What is the number of units in 1 mole of any substance, according to Avogadro's constant (NA)?
    1.602 \times 10^{22}
    6.02 \times 10^{23}
    3.05 \times 10^{25}
    9.83 \times 10^{21}
    30s
  • Q8
    Calculate the volume of 3 moles of oxygen gas (O2) at room temperature and pressure. Use Rule 3 to find the volume of 3 moles of oxygen gas.
    72 liters (L)
    60 liters (L)
    48 liters (L)
    36 liters (L)
    30s
  • Q9
    Calculate the number of moles of chlorine gas (Cl2) present in a 50 grams sample. Use Rule 1 to determine the number of moles.
    0.75 moles
    2.10 moles
    3.25 moles
    1.39 moles
    30s
  • Q10
    What is the formula to calculate the number of moles (n) when given the number of units (N) and Avogadro's constant (NA)?
    Number of moles (n) = number of units (N) - Avogadro's constant (NA)
    Number of moles (n) = number of units (N) * Avogadro's constant (NA)
    Number of moles (n) = number of units (N) ÷ Avogadro's constant (NA) = number of units (N) ÷ 6.02 \times 10^{23}
    Number of moles (n) = number of units (N) + Avogadro's constant (NA)
    30s
  • Q11
    What is the Avogadro's constant (NA)?
    9.02 \times 10^{23}
    6.02 \times 10^{23}
    3.02 \times 10^{23}
    12.02 \times 10^{23}
    30s
  • Q12
    What is the volume of 2 moles of a gas at room temperature and pressure according to Avogadro's Law?
    12 liters
    48 liters
    36 liters
    24 liters
    30s
  • Q13
    How many moles are present in 72 grams of a substance with a relative atomic mass of 12?
    8 moles
    2 moles
    4 moles
    6 moles
    30s
  • Q14
    What is the number of moles in 3.01 × 10^23 units of a substance, according to Avogadro's constant?
    2 moles
    1 mole
    3 moles
    0.5 moles
    30s
  • Q15
    What is the mass of 3 moles of a substance with a molecular relative mass of 30?
    120 grams
    150 grams
    60 grams
    90 grams
    30s

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