Mass and Moles in Chemistry
Explore the fundamental concepts of mass and moles in chemistry with this Grade 9 worksheet, covering atomic mass, molar mass, and mole calculations.
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Mass and Moles: Fundamental Chemistry
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Read each question carefully and answer to the best of your ability. Show all your work for calculation problems.
1. What is the approximate atomic mass of carbon?
1 amu
6 amu
12 amu
14 amu
2. Avogadro's number represents the number of particles in one of a substance.
gram
kilogram
mole
liter
3. The molar mass of a compound is the sum of the of all the atoms in its formula.
4. One mole of any substance contains approximately particles.
5. Calculate the molar mass of water (H₂O). (Atomic mass of H = 1.01 g/mol, O = 16.00 g/mol)
6. How many moles are present in 49.0 grams of sulfuric acid (H₂SO₄)? (Atomic mass of H = 1.01 g/mol, S = 32.07 g/mol, O = 16.00 g/mol)
7. The atomic mass unit (amu) is always equal to one gram.
True
False
8. The molar mass of an element is numerically equal to its atomic mass.
True
False
Match the term with its definition.
9. Mole
a. The mass of one mole of a substance
10. Molar Mass
b. 6.022 x 10²³ particles
11. Atomic Mass Unit
c. Unit used to express atomic and molecular masses
12. A sample of gas contains 3.01 x 10²³ molecules. If the gas is methane (CH₄), what is the mass of the sample in grams? (Atomic mass of C = 12.01 g/mol, H = 1.01 g/mol)