Unit 4 Review Questions

The atom that serves as the relative standard for determining mass and the number of particles in a mole is:
1. hydrogen-1
2. carbon-12
3. oxygen-16
4. lead-206
The amount of substance having 6.02 x 10²³ of any kind of chemical unit is called a(n):
1. atomic weight
2. mole
3. formula
4. mass number
The molar mass of sodium oxide, Na₂O is approximately
1. 55 grams
2. 39 grams
3. 62 grams
4. 6.022 x 10²³ grams
The mass of three moles of sodium oxide, Na₂O is approximately
1. 20 grams
2. 108 grams
3. 186 grams
4. 165 grams
How many moles of sodium oxide, Na₂O are in 310 grams of the compound?
1. 4 moles
2. 2 moles
3. 5 moles
4. 3 moles
The molar mass of butane, C₄H₁₀ is approximately:
1. 58 grams
2. 13 grams
3. 22 grams
4. 48 grams
The balanced equation for the combustion of butane, C₄H₁₀ is
2 C₄H₁₀ + 13 O₂ → 8 CO₂ + 10 H₂O

When 100 grams of butane is burned in an excess of oxygen,
1. the mass of CO₂ produced is greater than the mass of H₂O produced
2. the mass of CO₂ produced is less than the mass of H₂O produced
3. the mass of CO₂ produced is the same as the mass of H₂O produced
The balanced equation for the combustion of butane, C₄H₁₀ is
2 C₄H₁₀ + 13 O₂ → 8 CO₂ + 10 H₂O

Of the reactants and products in the combustion of butane,
1. all of them are ionic compounds
2. all of them are covalent molecules
3. two are ionic, and two are covalent
4. three are covalent, and one is ionic
What is the mass of two moles of gas propane gas, C₃H₈?
1. 44 grams
2. 88 grams
3. 22 grams
4. 36 grams
How many moles of propane gas, C₃H₈, are contained in 11 grams of the gas?
1. 0.25 moles
2. 4 moles
3. 2 moles
4. 484 moles
Water can be decomposed by elecrolysis. The balanced equation for the decomposition of water is
2 H₂O → 2H₂ + O₂

If 100 grams of water is decomposed, what is the total mas of hydrogen and oxygen formed?
1. 100 grams
2. 4 moles
3. 2 moles
4. 484 moles
Water can be decomposed by elecrolysis. The balanced equation for the decomposition of water is
2 H₂O → 2H₂ + O₂

If 100 grams of water is decomposed, which product will have the greater mass at collection?
1. Hydrogen will have more mass than the oxygen
2. Oxygen will have more mass than the hydrogen
3. Hydrogen and oxygen will have the same mass
Water can be decomposed by elecrolysis. The balanced equation for the decomposition of water is
2 H₂O → 2H₂ + O₂

If 18 grams of water is decomposed, what mass of hydrogen gas is formed?
1. 2 grams
2. Oxygen will have more mass than the hydrogen
3. Hydrogen and oxygen will have the same mass
Water can be decomposed by elecrolysis. The balanced equation for the decomposition of water is
2 H₂O → 2H₂ + O₂

If 18 grams of water is decomposed, what mass of oxygen gas is formed?
1. 16 grams
2. 32 grams
3. 18 grams
4. 2 grams
What is the mass of 4 moles of hydrogen molecules (H₂)?
1. 8 grams
2. 32 grams
3. 18 grams
4. 2 grams
About how many molecules of hydrogen, H₂, are present in 2 grams of hydrogen?
1. 2 molecules
2. 3 moles
3. 2/3 moles
4. 2 moles
How many moles of water molecules, H₂O, are present in a 27 gram sample of water?
1. 1.5 moles
2. 3 moles
3. 2/3 moles
4. 2 moles
How many moles of methane molecules, CH₄, are in 80 grams of methane?
1. 5 moles
2. 5.6 moles
3. 4 moles
4. 28 moles
About how many moles of helium would be found in 2 grams of helium?
1. 0.5 moles
2. 5.6 moles
3. 4 moles
4. 28 moles
When calcium burns in oxygen, it forms calcium oxide. The balanced equation is
2 Ca + O₂ → 2CaO

What mass of calcium must be burned in order to produce 56 grams of calcium oxide?
1. 40 grams
2. 5.6 moles
3. 4 moles
4. 28 moles
When calcium burns in oxygen, it forms calcium oxide. The balanced equation is
2 Ca + O₂ → 2CaO

What mass of oxygen is necessary to completely burn 80 grams of calcium?
1. 32 grams
2. 5.6 moles
3. 4 moles
4. 28 moles
When calcium burns in oxygen, it forms calcium oxide. The balanced equation is
2 Ca + O₂ → 2CaO

In this reaction,
1. one of the substances involved is an ionic compound
2. 16 gram
3. 64 grams
4. 8 grams
When calcium burns in oxygen, it forms calcium oxide. The balanced equation is
2 Ca + O₂ → 2CaO

Which of the following describes the reactants?
1. calcium is an alkali metal and oxygen is a nonmetal
2. 16 gram
3. 64 grams
4. 8 grams
When calcium burns in oxygen, it forms calcium oxide. The balanced equation is
2 Ca + O₂ → 2CaO

During the formation of calcium oxide
1. calcium loses two electrons and oxygen gains two electrons
2. calcium gains two electrons and oxygen loses two electrons
3. calcium loses one electron and oxygen gains one electron
4. calcium gains one electron and oxygen loses one electron
Al + O₂ → Al₂O₃

When the equation above is correctly balanced, the coefficient on Al is:
1. 1
2. calcium gains two electrons and oxygen loses two electrons
3. calcium loses one electron and oxygen gains one electron
4. calcium gains one electron and oxygen loses one electron
5. 5
Al + O₂ → Al₂O₃

When the equation above is correctly balanced, the coefficient on O₂ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
Al + O₂ → Al₂O₃

When the equation above is correctly balanced, the coefficient on Al₂O₃ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
H₂ + N₂ → NH₃

When the equation above is correctly balanced, the coefficient on H₂ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
H₂ + N₂ → NH₃

When the equation above is correctly balanced, the coefficient on N₂ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
H₂ + N₂ → NH₃

When the equation above is correctly balanced, the coefficient on NH₃ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
C₂H₂ + O₂ → CO₂ + H₂O

When the equation above is correctly balanced, the coefficient on C₂H₂ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
C₂H₂ + O₂ → CO₂ + H₂O

When the equation above is correctly balanced, the coefficient on O₂ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
C₂H₂ + O₂ → CO₂ + H₂O

When the equation above is correctly balanced, the coefficient on CO₂ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
C₂H₂ + O₂ → CO₂ + H₂O

When the equation above is correctly balanced, the coefficient on H₂O is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
Na + H₂O → NaOH + H₂

When the equation above is correctly balanced, the coefficient on Na is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
Na + H₂O → NaOH + H₂

When the equation above is correctly balanced, the coefficient on H₂O is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
Na + H₂O → NaOH + H₂

When the equation above is correctly balanced, the coefficient on NaOH is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
Na + H₂O → NaOH + H₂

When the equation above is correctly balanced, the coefficient on H₂ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
Ni(ClO₃)₂ → NiCl₂ + O₂

When the equation above is correctly balanced, the coefficient on Ni(ClO₃)₂ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
Ni(ClO₃)₂ → NiCl₂ + O₂

When the equation above is correctly balanced, the coefficient on NiCl₂ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
Ni(ClO₃)₂ → NiCl₂ + O₂

When the equation above is correctly balanced, the coefficient on O₂ is:
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6