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— pick one card, then click its partner (in the other column).
Definitions
A
Number of particles in exactly 12 g of carbon-12 (6.022 × 1023)
B
Mass in grams of one mole of a substance
C
Amount of substance containing 6.022 × 1023 entities
D
Ratio of moles of one substance to another in a balanced equation
E
Volume of one mole of any gas at STP (22.7 L)
F
Written description of a reaction using formulas and coefficients
G
A conversion factor that relates grams to moles
Mole-map conversion problems
Solve each with dimensional analysis, then click to check.
Mole map: mass (g) ⇆ moles ⇆ particles • volume of gas at STP (L) ⇆ moles with 22.7 L/mol
Problem 1
How many moles in 54.0 g of H2O?
H2O molar mass = 18.02 g/mol
ANSWER
54.0 g × (1 mol / 18.02 g) = 3.00 mol
Problem 2
How many molecules in 0.250 mol of CO2?
ANSWER
0.250 mol × 6.022 × 1023 = 1.51 × 1023 molecules
Problem 3
What is the mass of 1.50 mol of NaCl?
NaCl molar mass = 58.44 g/mol
ANSWER
1.50 mol × 58.44 g/mol = 87.7 g
Problem 4
How many moles in 45.4 L of helium at STP?
ANSWER
45.4 L × (1 mol / 22.7 L) = 2.00 mol