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Q1: What is the molar mass of an element?
A1: The mass of one mole of an element in grams per mole (g/mol), numerically equal to its atomic mass.
Q2: What is a mole in chemistry?
A2: A unit representing
6.022
×
10
23
6.022×10
23
particles (atoms, molecules, ions, etc.).
Q3: What is Avogadro's number?
A3:
6.022
×
10
23
6.022×10
23
, the number of particles in one mole.
Q4: What is the formula to calculate moles from mass?
A4: Moles = mass (g) ÷ molar mass (g/mol)
Q5: What is the formula to calculate mass from moles?
A5: Mass = moles × molar mass
Q6: What is the formula to calculate molar mass from mass and moles?
A6: Molar mass = mass ÷ moles
Q7: How many moles are in 36 g of water (H₂O)?
A7: 2.00 moles (Molar mass = 18 g/mol, 36 ÷ 18 = 2)
Q8: How many grams are in 3 moles of carbon dioxide (CO₂)?
A8: 132.0 g (Molar mass = 44 g/mol, 3 × 44)
Q9: How many moles are in 100 g of sodium chloride (NaCl)?
A9: 1.71 mol (Molar mass = 58.44 g/mol, 100 ÷ 58.44)
Q10: How many atoms are in 2.00 mol of helium?
A10:
1.204
×
10
24
1.204×10
24
atoms (2 × Avogadro’s number)
🟩 FORMULA UNITS & MOLECULES
Q11: What is a formula unit?
A11: The simplest ratio of ions in an ionic compound.
Q12: How do you convert moles to formula units?
A12: Multiply moles by Avogadro’s number.
Q13: How do you find the number of formula units in 0.75 mol of NaCl?
A13:
4.52
×
10
23
4.52×10
23
formula units (0.75 × Avogadro’s number)
Q14: How many molecules are in 1.20 mol of H₂O?
A14:
7.23
×
10
23
7.23×10
23
molecules
Q15: How many moles are in
3.01
×
10
23
3.01×10
23
formula units of KBr?
A15: 0.500 mol
🟦 STEP-BY-STEP PRACTICE
Q16: What is the molar mass of Al₂S₃?
A16: 150.14 g/mol
Q17: How many moles are in 62.2 g of Al₂S₃?
A17: 0.4144 mol
Q18: How many formula units are in 62.2 g of Al₂S₃?
A18:
2.49
×
10