Description of the Mole Concept:
Here E means 10 raised to the power of 'x'. E is followed by the value of 'x'.
Suppose you were sent into the store to buy 36 eggs. When you picked them up you would get 3 boxes, each containing 12 eggs. You just used a mathematical device, called DOZEN, to simplify the process.
You might also be asked to obtain a GROSS of some item. This amount is known to contain 144 (12 dozen).
Chemist began to realize that numbers like 12 and 144 were much too small to use when working with individual parts of matter like atoms and molecules. They chose to use the term MOLE to represent amounts of matter that were applicable for them.
Keep in mind that this word MOLE is representative of an amount of something. Just as you can have a dozen eggs you can also have a dozen chairs, a dozen people, a dozen stars. So the scientist of the world can have a mole of water, a mole of sodium chloride, a mole of gold.
Now I need to show you the number associated with the mole:
602,000,000,000,000,000,000,000
That large a number is difficult to use in calculations so we must use another mathematical shorthand, scientific notation, to help us.
Lets rewrite that same number as: 6.02 E 23
Another name for this huge amount: Avogadro's Number.
As it turns out this number, named after Amadeo Avogadro, is used as a reference point for most calculations and equations found in chemistry.
The next section on the main menu deals with the 4 general rules associated with the MOLE concept. These rules allow us to compare mass with volume, mass with number of particles, and balance chemical equations.
Rules Utilized With MOLE:
1. The chemical formula represents a mole of that substance.
2. The formula mass, expressed in grams, represents the mass of one mole of that substance.
3. One mole of any substance contains 6.02 E 23 particles.
4. One mole of any gas, at STP conditions, occupies 22.4 litres of volume.
Rule: The chemical formula represents a mole of that substance.
Remember that any number placed to the left of a chemical symbol or formula is called the COEFFICIENT. This number (integer, decimal, or in scientific notation) tells us the number of moles of that substance.
Examples: Pb à 1 mole of lead atoms (understood 1)
3 Pb à 3 moles of lead atoms
4.5 Cl à 4.5 moles of chlorine atoms
2 CaCl à 2 moles of calcium chloride
3.5 NaOH à 3.5 moles of sodium hydroxide
Rule: The formula mass, in grams, represents the mass of that substance.
The formula mass of an element is its atomic mass (found on Periodic Table.) The formula mass of a compound is found by multiplying the number of moles of that element (see its subscript in the formula) by that atom's atomic mass. Then add masses of all elements and record in grams.
The following example is given to demonstrate how to find formula mass.
CaCO3 (calcium carbonate)
Ca 1 x 40.1 = 40.1 C 1 x 12.0 = 12.0 O 3 x 16.0 = 48.0 ---- 100.1 grams = 100. g (3 significant figs)
If you need further help finding formula masses please see your teacher.
Now for some examples involving this rule:
2 Cu à 2 moles of copper atoms à 2 x 63.5 = 127
5.00 NaCl à 5 moles sodium chloride à 5.00 x 58.4 = 292 g
2.5 H2SO4 2.5 moles of sulphuric acid à 2.5 x 98.1 = 245 g
Rule: One mole of any substance contains 6.02 E 23 particles.
Particles here might mean atoms, molecules, ions, electrons, or just about anything you might need to work with. Remember: just as there are 12 items in a dozen; 6.02 E 23 particles in a mole.
Examples:
HNO3 à 1 mole of nitric acid, 1.00 x 63.0 = 63.0 grams, 6.02 E 23 molecules of nitric acid
3.00 K à 3.00 moles of potassium atoms , 3.00 x 39.1 = 117 grams, 3.00 x 6.02 E 23 =1.81 E 24 potassium atoms
Rule: One mole of any gas, at STP conditions, occupies 22.4 L of volume.
STP is a shorthand way of requiring the temperature to be at 0 degrees C and a standard pressure of 1 atm (101.3 kPa).
This rule is most commonly used when studying gas laws. Suppose you have 4 grams of helium gas. This represents 1 mole of helium (see 2nd rule). These 6.02 E 23 atoms of helium would take up 22.4 liters of volume. This large volume would be fully occupied if the temperature was 0 degrees Celsius and the pressure 1 atmosphere. A change in the temperature/pressure would, of course, change the volume occupied by the gas.
Sample Mole Calculations:
1)Formula to Number of Moles
Given: 4.50 Na2CO3 : how many moles of sodium carbonate are their
Remember: The coefficient in front of an element or compound tells you the number of moles you have .
Of course you were dealing with 4.50 moles of sodium carbonate.
Remember that the coefficient can be a whole number, decimal, a number in scientific notation, and that the number of significant figures in that coefficient indicates the degree of precision needed in your final answer.
2)Number of Moles to Formula
Given: 3.5 E-2 moles of calcium chloride, correctly represent the coefficient and formula:
The answer would be 3.5 E-2 CaCl2
3)Moles to Grams
Given: 2.00 moles of Ca(OH)2 would represent ________ grams.
Remember that 1 mole of a compound is represented by the formula mass of that compound. Also, 1 mole of an element equals the atomic mass.
To solve this problem we must first calculate the formula mass and then multiply that number by the number of moles we have (in this case: 2.0)
To calculate formula mass, first list the elements in the formula along with the number of each (hint: use the subscripts). Then multiply that number by the atomic mass of that element. Add those masses and you have the formula mass. Remember to get your final answer you must multiply the formula mass by the number of moles.
Calculate formula mass: Ca 1 x 40.1 = 40.1 O 2 x 16.0 = 32.0 H 2 x 1.01 = 2.02 ------ formula mass --> 74.1 g (rounded)
Calculate mass of 2.00 Ca(OH)2
2.00 x 74.1 g = 148 g (again rounded to 3 significant figures
4)Grams to Moles
Given: 48.5 grams of CaCO3 = ___________ moles of calcium carbonate
Remember that you must first find the formula mass of the compound.
Calculate formula mass: Ca 1 x 40.1 = 40.1 C 1 x 12.0 = 12.0 O 3 x 16.0 = 48.0 -------- formula mass -> 100. g (rounded)
Some of you will readily see that we have less than a full mole and simply divide 48.5/100. to get your answer.
5)Moles to Particles (Atoms, molecules, ions,...)
Given: 4.20 moles of hydrogen fluoride = _______ molecules HF
Remember that 1 mole of any thing has 6.02 E 23 particles.
So to answer this problem we would just multiply 4.20 x 6.02 E 23 and get the answer 2.53 E 24 molecules.
6)Grams to Particles
Given: 126 g of Lithium Sulphate = _______________ ion pairs Lithium Sulphate
We will need to calculate formula mass for lithium sulphate.Did you get 110. grams? Also we will need to remember that 6.02 E 23 ion pairs of lithium sulphate equals 1 mole.
Since 6.02 E 23 ion pairs equals 1 mole and 110. g of lithium sulphate equals one mole they are equal to each other. When we place two items that are equal to each other in a ratio it is equal to 1.
Moles- Avogadro's Number
1. The chemical formula represents 1 mole of that substance.
2. The formula mass (expressed in grams) is the mass of 1 mole of that substance.
3. 1 mole of a substance contains 6.02 E 23 particles (atoms, molecules, ions, electrons, etc.)
4. 1 mole of any gas at STP (1 atmosphere of pressure and 0 °C) occupies 22.4 liters of volume.
Atomic nitrogen(N)=14.0 g=6.02 E 23 atoms
Nitrogen gas (N2)= 28.0 g=6.02 E 23 molecules (1.20 E 24 atoms)
Silver ions(Ag+1)=108 g=6.02 E 23 ions
Sodium chloride(NaCl)=58.5 g=6.02 E 23 ion pairs
Ammonium sulphate[(NH4)2SO4]=132 g=6.02 E 23 molecules
Problems:
1 mole Ca = _________ g
1 mole MgSO4 = _________ atoms
7 moles H2= _________ g
7 moles FeCl2= _________ atoms
0.5 mol CO2 = ________g = ___________ molecules
1.5 mol MgCl2 = _________g = ___________ ion pairs
1 mol KNO3 = _________ mol K, _________ mol N, ________mol O
1 mol KNO3 = _________ g K, __________g N, ___________ g O
10 g KNO3 = __________ mol KNO3, __________ g K, ___________ atoms O
2.2 mol of H3PO4 there are ___________ g H, __________mol p, __________atoms O
Molarity
Molarity: the ratio between the moles of dissolved substance (solute) and the volume of the solution (in liters or cubic decimeters)
Example: 1 M HNO3 = 1 mole of HNO3 in 1 L of solution
0.273 M Ba(NO3)2 contains 0.372 moles of barium nitrate in 1 L of solution
Problems:
1. 145 g (NH4)2C4H4O6 in 500 mL of solution
3. 45.1 g cobalt (II) sulphate in 250 mL of solution
4. 41.3 g iron (II) nitrate in 100 mL solution
5. 49.9 g Pb(ClO4)2 in 200 mL of solution
Sample test problems:
1. 22 E 4 grams of carbon (IV) oxide contains ________grams of oxygen
2. 56 E ? 15 moles of carbon (II) oxide contains _________ atoms of carbon
3. 5.50 E 16 atoms of zinc weighs _________ grams
4. 5.50 E 16 atoms of manganese is _________ moles of manganese
5. 8.35 moles of chromium sulphate weighs __________ grams.
6. 8.35 moles of ozone contains _________atoms of oxygen
PHYSICAL SCIENCE WORKSHEET
1. 1 mole of iron weighs ____________________ grams.
2. 1 mole of iron contains __________________ atoms.
3. 7.4 moles of iron weighs _________________ grams.
4. 7.4 moles of iron contains _________________ atoms.
5. 1 gram of iron contains __________________ atoms.
6. 1 atom of iron weighs ____________________ grams.
7. 1.2 E 24 atoms of iron would be _________________ moles of iron.
8. 6.4 E 31 atoms of iron would be __________________ moles of iron.
9. 6.4 E 31 atoms of iron weighs ____________________ grams.
10. 140 grams of iron would be _______________________ atoms.
11. 1 mole of Ca(OH)2 weighs _______________________ grams.
12. In one mole of Ca(OH)2 there are __________________ ion pairs.
13. 4 moles of Ca(OH)2 weighs ____________________ grams.
14. In 2.2 E - 3 moles of Ca(OH)2 there are _________________ ion pairs.
15. The total number of atoms in one mole of Ca(OH)2 would be _____________.
16. 2.2 E - 3 moles of Ca(OH)2 weighs ________________ grams.
17. 1.6 E 4 grams of Ca(OH)2 would would be ____________________ ion pairs.
18. A compound contains 29.1% sodium, 40.5% sulphur, and 30.4% oxygen.
What would be the empirical formula for this compound? _______________
19. 3 grams of hydrogen combines with 42 grams of nitrogen and 144 grams of oxygen to form a new compound. What would be the empirical formula of this compound? _________ How many moles of this compound would be created? _______.
20. Describe how you could make (exactly) 183 grams of KClO3.
PHYSICAL SCIENCE WORKSHEET
1. 1 mole of CO2 weighs _____________________ grams.
2. 3 moles of CO2 contains __________________ molecules of CO2.
3. 3 molecules of CO2 weighs ________________ grams.
4. 3 moles of CO2 contains __________________ atoms of carbon.
5. 3.1 moles of CO2 contains ________________ molecules of CO2.
6. 3.1 moles of CO2 contains ________________ grams of CO2.
7. 1 mole of KClO3 weighs ___________________ grams.
8. 6 grams of KClO3 would be ________________ moles.
9. 6 grams of KClO3 if split up will produce ___________ grams of K,
____________ grams of Cl, and ___________ grams of O.
10. Find the percentage composition of each element in KNO3.
______________% K, _____________% N, _____________% O
11. 1 mole of KNO3 weighs ________ grams and contains ___________ ion pairs.
12. In 1 mole of KNO3 there are ____________ moles of K,
____________ moles of N, and 3 moles of _________________.
13. In 0.25 moles of KNO3 there are ___________ grams of K,
___________ grams of N, and ____________ grams of O.
14. 5 E 23 ion pairs of KNO3 is ___________ moles and weighs _________ grams.
15. 10 grams of KNO3 would be ____________ moles of KNO3 and would be
________________ ion pairs.
16. In 2.2 moles of H3PO4 there are __________ grams of H,
___________ grams of P, and _____________ grams of O.
17. 2.1 E 24 molecules of H3PO4 would be ______________ moles and would
weigh ____________ grams.
18. In 2.2 moles of H3PO4 there are _________________ molecules of H3PO4
and ________ atoms of H, _________ atoms of P, and _________ atoms of O
19. In 100 grams of H3PO4 there would be __________ grams of H,
___________ grams of P, and ___________ grams of O.
20. Find the percentage composition of each element in H3PO4
_____________% H, ______________% P, _______________% O
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