Density
Specific Heat
Empirical/Molecular Formula
Stoichiometry
100
What is the formula for density?

D=m/V

100

What is the formula for specific heat?

q=mCsT

100

This is the simplest whole-number ratio of elements in a compound.

Empirical Formula

100

Given the balanced equation:

2H2+O2 -> 2H2O

If you start with 4 moles of H2, how many moles of water will be produced?

4 moles of water

200

A metal block has a mass of 150 g and a volume of 50 cm2. What is the density of the metal block?

3.0 g/cm2

200

What is the specific heat of water?

4.184 J/goC

200

The empirical formula of C6H12O6

CH2O

200

How many grams of carbon dioxide are produced from the complete combustion of 88 g of propane (C3H8).

132 g of carbon dioxide

300

A substance will float in water if its density is less than this value.

1.0 g/mL

300

This is the amount of heat required to raise 10 g of iron (c = 0.45 J/g°C) by 20°C.

90 J

300

A compound has 40% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. This is its empirical formula.

CH2O

300

How many liters of oxygen gas (O2) at STP are needed to react with 5 moles of hydrogen gas (H2) in the reaction below?

2H2+O2 -> 2H2O

56.0 L of O2

400

A gas at STP has a density of 1.25 g/L. Given that D=m/V, this is the molar mass of the gas.

28.0 g/mol

400

When heat is added to a system but temperature doesn’t change, this phase transition might be occurring.

Melting or boiling

400

A compound has an empirical formula of CH and a molar mass of 78 g/mol. This is its molecular formula.

C6H6

400

If you have 50 g of aluminum (Al) reacting with excess oxygen (O2), how many grams of aluminum oxide (Al2O3) can be produced?

94.4 g of Al2O3

500

The density of a liquid changes with this property due to molecular expansion

Due to temperature.

500

The reason metals have lower specific heat values compared to water.

What is their lower capacity to store heat energy per unit mass?

500

Given that the molecular formula is always a multiple of the empirical formula, this is the molecular formula of a compound with an empirical formula of NO2 and a molar mass of 92 g/mol.

N2O4

500

How many molecules of water are produced when 10 g of hydrogen gas reacts with excess oxygen?

3.0 x 1024 molecules of H2O