the atoms of a molecular formula shown in the smallest ratio
100
What is a molecular formula?
the chemical formula with atoms in the ratios they actually occur
100
What is a hydrate?
a salt with water bonded to the ions in the crystal structure
200
What element was the mole derived from?
carbon-12 (the number of atoms in 12g of carbon-12)
200
How many moles are there in 76.44 g H3PO4?
0.78 mol
200
What is the empirical formula for carbon monoxide?
CO
200
What is the molecular formula for copper II sulfate?
CuSO4
200
What is the name for BaCl2•2H2O
barium chloride dihydrate
300
Which scientist is responsible for our use of the mole?
Avagadro
300
How many grams are in 6.2 mol BF3?
420.36g
300
What is the empirical formula for glucose? (C6H12O6)
CH2O
300
What are the steps you must follow to find the molecular formula?
find the empirical formula (using the "rhyming steps")
calculate the empirical formula mass
divide the molar mass by the empirical formula mass
multiply the empirical formula by this number
300
What is the name for FeSO4•6H2O?
iron II sulfate hexahydrate
400
Name 3 "representative particles" the mole can be used to count.
atoms, molecules, formula units, ions
400
How many representative particles are in 35.4 mol CO2?
2.13x10^25 molecules
400
What is the rhyme to help you remember the steps to finding the empirical formula?
percent to mass
mass to mole
divide by small
multiply by whole
400
Find the molecular formula for a compound whose molar mass is 124.06 and empirical formula is CH2O3.
C3H4O2
400
A substance that absorbs water from the air is _____________.
hygroscopic
500
Why do we use the mole in chemistry?
it is used as a counting unit because individual atoms or molecules are far too small to work with by themselves
500
Why can't you convert directly from particles to grams(and vice versa)?
You have to convert to moles first
500
What is the empirical formula for a compound containing 50.0% C, 5.5% H, and 44.4% O?
C3H4O2
500
What is the empirical formula of a compound containing 65.0% Cr and 35.0%O?
Cr4O7
500
A 15.67 g sample of a hydrate of magnesium carbonate was heated to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate?