Chapter 6: Stoichiometery

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1. Which law forms the basis of stoichiometry?

A Law of inertia

B Law of conservation of mass

C Law of motion

D Law of gravitation

2. Fatima is writing the chemical formula for sodium oxide. Sodium has a +1 charge and oxide has a -2 charge. What is the formula?

A NaO

B Na2O

C NaO2

D Na2O2

3. Ming is studying empirical and molecular formulas. He knows that the empirical formula is the simplest ratio of atoms, while the molecular formula is the actual number. For a compound with empirical formula CH and molecular mass 78, what is the molecular formula? (C=12, H=1)

A C6H6

B C2H2

C C3H3

D C4H4

4. Julia is studying gram formula mass. She wants to find the gram formula mass of CaCl2. (Ca=40, Cl=35.5)

A 75.5 g

B 111 g

C 90.5 g

D 120 g

5. Nora is calculating the number of atoms in 2 moles of helium. How many atoms are there?

A 1.204 × 10^24 atoms

B 6.022 × 10^23 atoms

C 3.011 × 10^23 atoms

D 1.806 × 10^24 atoms

6. Stoichiometric calculations are based on:

A Unbalanced equations

B Balanced equations

C Word equations

D Skeletal equations

7. Which step is necessary before stoichiometric calculations?

A Writing word equation

B Balancing equation

C Finding temperature

D Measuring volume

8. Molecular formula shows:

A Simplest ratio of atoms

B Percentage composition

C Actual number of atoms

D Ionic charge

9. The molar mass of H2O is:

A 16 g/mol

B 17 g/mol

C 18 g/mol

D 20 g/mol

10. The mole is a unit used to measure:

A Mass

B Volume

C Amount of substance

D Density

Chapter 6: Stoichiometery

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