The Mole Understanding and Practice
12-06-11
Remember that the mole is a word that has a certain numerical value. This number of
particles is equal to certain other values that can actually be measured in the laboratory.
1.
How many particles (atoms) are in 1.35 moles of Sodium (Na)?
2.
How many particles (molecules) are in 2.45 moles of Carbon Dioxide (CO2)?
3.
What number of moles does a student have if they have 4.33 X 1026 formula units of
Sodium Chloride (NaCl)?
4.
What number of moles are in 8.00 x 1020 atoms of Aluminum (Al)?
5.
What is the molar mass of Calcium Sulfate (CaSO4)?
If the student has 67.80 g of CaSO4, what number of moles do they have ?
6.
What is the molar mass of Ammonium Nitrate (NH4NO3)?
What number of moles does the student have if they measure 78.40 g of NH4NO3 into
a beaker?
7.
What is the molar mass of glucose (C6H12O6)?
What mass of glucose is equal to 0.376 moles?
8.
What is the molar mass of Copper (II) phosphate?
What mass of Copper (II) Phosphate is equal to 0.056 32 moles?
9.
What volume will oxygen gas (O2) at STP occupy if it is a total of 4.00 liters?moles?
10.
How many moles of gas at STP will Ammonia (NH3) gas occupy in liters be if it occupies
0.738 liters?
11.
How many moles of Carbon Dioxide gas are in a container that is 6.25 liters, if at STP?
12.
If a flexible container has 0.0349 moles of gas at STP, what is the volume of the
container in liters?