Section 1
Section 2
Section 3
Section 4
Section 5
100
What is the SI base unit used to measure the amount of a substance?
The Mole
100
What is the mass in grams of mole of any pure substance?
Molar Mass
100

What is the mass of 5.0 x 1021 molecules of water?

0.15 g of water

100
What relationship is described by the formula below? (mass of the element/mass of the compound) x 100
Percent Composition
100

The term used for a compound that has a specific number of waters bonded to it.

Hydrate

200

What does the number 6.022 x 10^23 represent?

Avogadro's Number

200
The Molar Mass of any element is numerically equivalent to its atomic mass and has the unit ___?
g/mol
200

What is the mass of 1.0 x 1012 molecules of O2?

5.3 x 10-11 grams of molecules

200
How can the actual molecular formula be determined?
From the molar mass divided by the mass of the empirical formula
200

When all the water has been lost from the substance and only the compound is left. 

Anhydrate

300

1 mole= (?) Molecules and 1 mole= (?) of the element

6.022 x 10^23 Molecules 

Molar Mass of the Element

300
Easy Practice: 1 mole of C atoms= (?) 1 mole Mg atoms = (?) 1 mole of Cu atoms = (?)
1 mole of C atoms= 12.0 grams 1 mole Mg atoms = 24.3 grams 1 mole of Cu atoms = 63.5 grams
300

How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH3?

6.0 mol

300

Analysis of a covalent compound showed that it contained 14.4% hydrogen and 85.6% carbon by mass. What is the empirical formula for this compound?

CH2

300

What is the mass of 1.000 mole of carbon atoms?

12.01 grams

400

Convert 2.3 x 1032 particles to moles of nitrogen.

3,819,329,127 moles or 3.819 x 10moles

400

Convert Moles to Mass 1.25 moles of Nitrogen=____ grams

35.0 grams (since Nitrogen is diatomic multiply AMU by 2)

400

What is the molar mass of H2CrO4?

118 g

400

A sample of liquid contains 0.059% hydrogen and 0.94% oxygen. What is the empirical formula?

HO

400

Determine the hydrate formula from the following information.  If 1.951 g BaCl2 · nH2O yields 1.864 g of anhydrous BaCl2 after treatment with sulfuric acid, calculate n. 

BaCl2 · 2H2O

500

Convert 100 grams of C6H12O6 to molecules

3.341 x 1023 molecules

500

Convert 35.4 g of CuF2 to Atoms

2.06 x 1022 atoms

500

Acetic acid has the molecular formula CH3COOH. How many atoms of oxygen in 60 grams of acetic acid?

1.2 x 1024 atoms of oxygen

500

The empirical formula for a sample of liquid is HO. The molecular weight is 34.0 grams/mole. What is the molecular formula?

H2O2

500

Calculate the Hydrate formula based on the following information. A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate? 

MgCO3 · 5H3O

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