Choose the correct answer for each question.

- The atom that serves as the relative standard for determining mass and the number of particles in a mole is:
- hydrogen-1
- carbon-12
- oxygen-16
- lead-206

- The amount of substance having 6.02 x 10
^{23}of any kind of chemical unit is called a(n):- atomic weight
- mole
- formula
- mass number

- The molar mass of sodium oxide, Na
_{2}O is approximately- 55 grams
- 39 grams
- 62 grams
- 6.022 x 10
^{23}grams

- The mass of three moles of sodium oxide, Na
_{2}O is approximately- 20 grams
- 108 grams
- 186 grams
- 165 grams

- How many moles of sodium oxide, Na
_{2}O are in 310 grams of the compound?- 4 moles
- 2 moles
- 5 moles
- 3 moles

- The molar mass of butane, C
_{4}H_{10}is approximately:- 58 grams
- 13 grams
- 22 grams
- 48 grams

- The balanced equation for the combustion of butane, C
_{4}H_{10}is2 C_{4}H_{10}+ 13 O_{2}→ 8 CO_{2}+ 10 H_{2}O

When 100 grams of butane is burned in an excess of oxygen,- the mass of CO
_{2}produced is greater than the mass of H_{2}O produced - the mass of CO
_{2}produced is less than the mass of H_{2}O produced - the mass of CO
_{2}produced is the same as the mass of H_{2}O produced

- the mass of CO
- The balanced equation for the combustion of butane, C
_{4}H_{10}is2 C_{4}H_{10}+ 13 O_{2}→ 8 CO_{2}+ 10 H_{2}O

When an unknown quantity of butane is burned, 90 grams of water is collected. Based on the amount of water collected, what mass of butane was burned?- 58 grams
- 116 grams
- 29 grams
- 232 grams

- The balanced equation for the combustion of butane, C
_{4}H_{10}is2 C_{4}H_{10}+ 13 O_{2}→ 8 CO_{2}+ 10 H_{2}O

When an unknown quantity of butane is burned, 90 grams of water is collected. Based on the amount of water collected, what mass of carbon dioxide should have been collected at the same time?- 176 grams
- 88 grams
- 44 grams
- 352 grams

- The balanced equation for the combustion of butane, C
_{4}H_{10}is2 C_{4}H_{10}+ 13 O_{2}→ 8 CO_{2}+ 10 H_{2}O

Of the reactants and products in the combustion of butane,- all of them are ionic compounds
- all of them are covalent molecules
- two are ionic, and two are covalent
- three are covalent, and one is ionic

- What is the mass of two moles of propane gas, C
_{3}H_{8}?- 44 grams
- 88 grams
- 22 grams
- 36 grams

- How many moles of propane gas, C
_{3}H_{8}, are contained in 11 grams of the gas?- 0.25 moles
- 4 moles
- 2 moles
- 484 moles

- Water can be decomposed by elecrolysis. The balanced equation for the decomposition of water is2 H
_{2}O → 2H_{2}+ O_{2}

If 100 grams of water is decomposed, what is the total mass of hydrogen and oxygen formed?- 100 grams
- 200 grams
- 300 grams
- 50 grams

- Water can be decomposed by elecrolysis. The balanced equation for the decomposition of water is2 H
_{2}O → 2H_{2}+ O_{2}

If 100 grams of water is decomposed, which product will have the greater mass at collection?- Hydrogen will have more mass than the oxygen
- Oxygen will have more mass than the hydrogen
- Hydrogen and oxygen will have the same mass

- Water can be decomposed by elecrolysis. The balanced equation for the decomposition of water is2 H
_{2}O → 2H_{2}+ O_{2}

If 18 grams of water is decomposed, what mass of hydrogen gas is formed?- 2 grams
- 1 gram
- 4 grams
- 18 grams

- Water can be decomposed by elecrolysis. The balanced equation for the decomposition of water is2 H
_{2}O → 2H_{2}+ O_{2}

If 18 grams of water is decomposed, what mass of oxygen gas is formed?- 16 grams
- 32 grams
- 18 grams
- 2 grams

- What is the mass of 4 moles of hydrogen molecules (H
_{2})?- 8 grams
- 32 grams
- 18 grams
- 2 grams

- About how many molecules of hydrogen, H
_{2}, are present in 2 grams of hydrogen?- 6 x 10
^{23}molecules - 2 molecules
- 1 molecule
- 18 molecules

- 6 x 10
- How many moles of water molecules, H
_{2}O, are present in a 27 gram sample of water?- 1.5 moles
- 3 moles
- 2/3 moles
- 2 moles

- How many moles of methane molecules, CH
_{4}, are in 80 grams of methane?- 5 moles
- 5.6 moles
- 4 moles
- 28 moles

- About how many moles of helium would be found in 2 grams of helium?
- 0.5 moles
- 5.6 moles
- 4 moles
- 28 moles

- When calcium burns in oxygen, it forms calcium oxide. The balanced equation is2 Ca + O
_{2}→ 2CaO

What mass of calcium must be burned in order to produce 56 grams of calcium oxide?- 40 grams
- 56 grams
- 20 grams
- 80 grams

- When calcium burns in oxygen, it forms calcium oxide. The balanced equation is2 Ca + O
_{2}→ 2CaO

What mass of oxygen is necessary to completely burn 80 grams of calcium?- 32 grams
- 16 gram
- 64 grams
- 8 grams

- When calcium burns in oxygen, it forms calcium oxide. The balanced equation is2 Ca + O
_{2}→ 2CaO

In this reaction,- one of the substances involved is an ionic compound
- none of the substances is covalently bonded
- all of the substances are covalently bonded
- mass is converted to energy

- When calcium burns in oxygen, it forms calcium oxide. The balanced equation is2 Ca + O
_{2}→ 2CaO

Which of the following describes the reactants?- calcium is an alkali metal and oxygen is a nonmetal
- calcium is an alkaline earth metal and oxygen is a nonmetal
- calcium is a transition metal and oxygen is a nonmetal
- calcium is an alkali metal and oxygen is a halogen

- When calcium burns in oxygen, it forms calcium oxide. The balanced equation is2 Ca + O
_{2}→ 2CaO

During the formation of calcium oxide- calcium loses two electrons and oxygen gains two electrons
- calcium gains two electrons and oxygen loses two electrons
- calcium loses one electron and oxygen gains one electron
- calcium gains one electron and oxygen loses one electron

- Al + O
_{2}→ Al_{2}O_{3}

When the equation above is correctly balanced, the coefficient on Al is:- 1
- 2
- 3
- 4
- 5

- Al + O
_{2}→ Al_{2}O_{3}

When the equation above is correctly balanced, the coefficient on O_{2}is:- 1
- 2
- 3
- 4
- 5
- 6

- Al + O
_{2}→ Al_{2}O_{3}

When the equation above is correctly balanced, the coefficient on Al_{2}O_{3}is:- 1
- 2
- 3
- 4
- 5
- 6

- H
_{2}+ N_{2}→ NH_{3}

When the equation above is correctly balanced, the coefficient on H_{2}is:- 1
- 2
- 3
- 4
- 5
- 6

- H
_{2}+ N_{2}→ NH_{3}

When the equation above is correctly balanced, the coefficient on N_{2}is:- 1
- 2
- 3
- 4
- 5
- 6

- H
_{2}+ N_{2}→ NH_{3}

When the equation above is correctly balanced, the coefficient on NH_{3}is:- 1
- 2
- 3
- 4
- 5
- 6

- C
_{2}H_{2}+ O_{2}→ CO_{2}+ H_{2}O

When the equation above is correctly balanced, the coefficient on C_{2}H_{2}is:- 1
- 2
- 3
- 4
- 5
- 6

- C
_{2}H_{2}+ O_{2}→ CO_{2}+ H_{2}O

When the equation above is correctly balanced, the coefficient on O_{2}is:- 1
- 2
- 3
- 4
- 5
- 6

- C
_{2}H_{2}+ O_{2}→ CO_{2}+ H_{2}O

When the equation above is correctly balanced, the coefficient on CO_{2}is:- 1
- 2
- 3
- 4
- 5
- 6

- C
_{2}H_{2}+ O_{2}→ CO_{2}+ H_{2}O

When the equation above is correctly balanced, the coefficient on H_{2}O is:- 1
- 2
- 3
- 4
- 5
- 6

- Na + H
_{2}O → NaOH + H_{2}

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

- Na + H
_{2}O → NaOH + H_{2}

When the equation above is correctly balanced, the coefficient on H_{2}O is:- 1
- 2
- 3
- 4
- 5
- 6

- Na + H
_{2}O → NaOH + H_{2}

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

- Na + H
_{2}O → NaOH + H_{2}

When the equation above is correctly balanced, the coefficient on H_{2}is:- 1
- 2
- 3
- 4
- 5
- 6

- Ni(ClO
_{3})_{2}→ NiCl_{2}+ O_{2}

When the equation above is correctly balanced, the coefficient on Ni(ClO_{3})_{2}is:- 1
- 2
- 3
- 4
- 5
- 6

- Ni(ClO
_{3})_{2}→ NiCl_{2}+ O_{2}

When the equation above is correctly balanced, the coefficient on NiCl_{2}is:- 1
- 2
- 3
- 4
- 5
- 6

- Ni(ClO
_{3})_{2}→ NiCl_{2}+ O_{2}

When the equation above is correctly balanced, the coefficient on O_{2}is:- 1
- 2
- 3
- 4
- 5
- 6