# Questions: Moles

### PROBLEM #1, SET 1 - MOLS

1. How many pennies are in a mole of pennies? How many thousand-dollar bills (k-notes!) is that mole of pennies equal to?

The first part of the problem is easy based on the definiton that a mol of ANYTHING is 6.023 E23 of them. A mol of pennies is 6.023 E23 pennies. This is what is GIVEN in the second part of the question. The second part is just a DA problem because we are going from one amount of money to another.

Pennies (E-2 dollars) to k-notes (E3 dollars) is a metric conversion. Just from the definitions of penny and k-note, we can say that 1kK-note = E5 pennies.

As for any DA problem, begin with what you know. There is no denominator for "GIVEN," so use "1." Use the definition as a conversion factor so you can cancel the units you don't want and leave the units you do.

E5 is 100,000. The calculator math is: 6.023 E23 ÷ 100000 =

The math for this problem is not spectacular. Aside from being a good reminder of how to do DA problems, the answer is important for its magnitude. Consider that if we had a mol of pennies, the value of them would be six billion (E9) times a billion (E9) thousand dollar bills(E5 pennies). This gives you some idea that the number for mol is so large that it is incomprehensible to most people. The ease of writing Avogadro's number in the scientific notation system gives us a sense of understanding that number that is really not there.

### PROBLEM #2, SET 1 - MOLS

2. NO2 is the molecular formula for nitrous dioxide (also known as nitrogen dioxide). List the information available to you from this formula.

The small formula NO2 has a lot of information in it. The most basic is that: (a) each formula of nitrous dioxide has one nitrogen atom and two oxygen atoms, (b) the formula weight is 46 g/mol (16 g/mol for each oxygen and 14 g/mol for the single nitrogen in each formula), and (c) the material makes molecules in which the atoms are attached by covalent bonds (because it is two non - metal elements).

(In answer to part a) Each element has one and only one capital letter. Nobelium has the symbol, "No." One capital letter, one element. Carbon monoxide, a compound of one carbon atom and one oxygen atom, is CO, but cobalt, the single atom of an element, is Co. The smaller subscript "2" after the "O" for oxygen indicates that there are two oxygen atoms in the formula. The numbers written in this way refer ONLY to the element just before it OR the group of elements inside the parentheses just before it, such as: Al2(SO4)3. In the aluminum sulfate formula the "2" shows two aluminum atoms, the "4" shows four oxygen atoms, and the "3" outside the parehtheses indicates three phosphates, that is, the entire contents of the parentheses must be multiplied by three. The total atom count for aluminum phosphate is two aluminum atoms, three sulfur atoms, and twelve (three times four) oxygen atoms.

(In answer to part b) One of the important lessons of this chapter is the finding of a formula weight. The formula weight is the mass in Atomic Mass Units of one entire formula or the number of grams of material based on the sum of the atomic weights of the atoms in a formula. (The phrase, "formula weight" is the more general term that inculdes the term, "molecular weight." Some materials just don't come in molecules.) The formula weight of a material can be found by adding the atomic weights of the atoms in the a formula of the material. In the case of NO2, there is one nitrogen at an atomic weight of 14.0 and two oxygen atoms at atomic weights of 16.0 each. When the formulas become larger, such as the blue vitriol in problem #4 m in this set, it might be a good idea to make a list of the atoms in the material such as:
1 Cu ---- 1 x 63.5 = 63.5 g/mol
1 S ------ 1 x 32.1 = 32.1 g/mol
4 O ----- 4 x 16.0 = 64.0 g/mol
10 H --- 10 x 1.0 = 10.0 g/mol
5 O ----- 5 x 16.0 = 80.0 g/mol
__________________________________
totals of 21 atoms and 249.6 g/mol in each formula.

(In answer to part c) A metal and a non-metal will usually form an ionic bond. An electron or several electrons from the metal leave the metal, forming a positive ion, and an electron or several electrons can be taken up by the non - metal to form a negativ ion. The resulting (+ and -) ions attract each other in what is called an ionic bond. But NO2 has not metal element in it. The two non - metals can only bond by sharing electrons in a covalent bond.

### PROBLEM #3, SET 1 - MOLS

3. C2H2 is the molecular formula for ethylyne (A.K.A. acetylene). (a) How many atoms are in one molecule? (b) Which atoms make up acetylene? (c) How many moles of atoms are in one molecule of acetylene? (d) How many molecules are in 5.3 moles of acetylene? (e) How many atoms are in a mole of acetylene?

(a) Acetylene has four atoms in each formula, two carbons and two hydrogens. It is a true molecule because it is held together by covalent bonds.

(b) Carbon and hydrogen only.

(c) There are four atoms in each molecule of acetylene, so there are 4/Avogadro's number of mols of atoms per molecule.
The math is:   4 ÷ 6.023 E 23 = 6.6412 E-24 mols of atoms per molecule

(d) Each mol of acetylene is 6.023 E23 molecules, so 5.3 mols is 5.3 X 6.023 E23 molecules of acetylene.
The math is:   5.3 x 6.023 E 23 = 3.1922 E 24 molecules

(e) Each mol of acetylene is 6.023 E23 molecules, and each molecule has four atoms, so there are 4 x 6.023 E23 atoms in a mol.
The math is:   4 x 6.023 E 23 = 2.4092 E 24 atoms per mol of acetylene

Back to mol problems.

### PROBLEM #4, SET 1 - MOLS

4. Calculate the molar mass of a mole of the following materials: (a) Al (b) Ra (c) Co (d) CO (e) CO2 (f) HCl (g) Na2CO3 (h) Ca(NO3)2 (i) (NH4)3(PO4) (j) H2O (k) Epsom salts - Mg(SO4)•7H2O (m) blue vitriol - Cu(SO4)•5H2O

All of these molar masses can be calculated with the help of a periodic chart with the atomic weight. The formula weight is the sum of the atomic weights of the atoms in a formula of the material. The units of formula weight or atomic weight or molecular weight is "grams per mol." Chemtutor calculates the formula weights by using the atomic weight of elements with ONE DIGIT to the right of the decimal point. Your instructor may use two or three digits to the right of the decimal point or some other method. It is common to calculate to the nearest whole number, but many elements have fractional numbers a significant portion of a whole number. In calculating one decimal to the right, the most significant deviation is that of hydrogen in organic compounds, not so much due to the significance of deviation of one atom, but that there are usually so many hydrogen atoms in oranic compounds.

(a) Al --- 1 x 27.0 = 27.0 g/mol

(b) Ra --- 1 x 226.0 = 226.0 g/mol

(c) Co --- 1 x 58.9 = 58.9 g/mol

(d) CO --- C --- 1 x 12.0 = 12.0 g/mol
O --- 1 x 16.0 = 16.0 g/mol
-----------------------------------------------
totals ----- 1 C and 1 O ---- 28.0 g/mol

(e) CO2 --C --- 1 x 12.0 = 12.0 g/mol
O --- 2 x 16.0 = 32.0 g/mol
-----------------------------------------------
totals ---- 1 C and 2 O ---- 44.0 g/mol

(f) NaCl -- Na --- 1 x 23.0 = 23.0 g/mol
Cl --- 1 x 35.5 = 35.5 g/mol
-----------------------------------------------
totals ---- 1 Na and 1 Cl ---- 58.5 g/mol

(g) Na2CO3 -- Na --- 2 x 23.0 = 46.0 g/mol
C --- 1 x 12.0 = 12.0 g/mol
O --- 3 x 16.0 = 48.0 g/mol
-----------------------------------------------
totals ----- 2 Na, 1 C, 3 O ----- 106.0 g/mol

(h) Ca(NO3)2 -- Ca --- 1 x 40.1 = 40.1 g/mol
N --- 2 x 14.0 = 28.0 g/mol
O --- 6 x 16.0 = 96.0 g/mol
-----------------------------------------------
totals ------ 1 Ca, 2 N, 6 O ------ 164.1 g/mol

(i) (NH4)3(PO4) -- N -- 3 x 14.0 = 42.0 g/mol
H ----- 12 x 1.0 = 12.0 g/mol
P ----- 1 x 31.0 = 31.0 g/mol
H ----- 4 x 16.0 = 64.0 g/mol
-----------------------------------------------
totals --------- 1 N and 3 H -------- 149.0 g/mol

(J) H2O -- H --- 2 x   1.0 =   2.0 g/mol
O --- 1 x 16.0 = 16.0 g/mol
-----------------------------------------------
totals ---- 2 H and 1 O ---- 18.0 g/mol

(k) Epsom salts, Mg(SO4)•7H2O
Mg ---   1 x 24.3 =   24.3 g/mol
S -----   1 x 32.1 =   32.1 g/mol
H ----- 14 x  1.0 =   14.0 g/mol
O ----- 11 x 16.0 = 176.0 g/mol
-----------------------------------------------
totals ---- 1 Mg, 1 S, 14 H, 11 O --- 246.4 g/mol

There is no "l," just as in Christmas.

(k) blue vitriol - Cu(SO(PO4)•5H2O
Cu ---   1 x 63.5 =   63.5 g/mol
S -----   1 x 32.1 =   32.1 g/mol
H ----- 10 x  1.0 =   10.0 g/mol
O -----  9 x 16.0 = 144.0 g/mol
-----------------------------------------------
totals ----- 1 Cu, 1 S, 10 H, 9 O ---- 249.6 g/mol

### PROBLEM #5, SET 1 - MOLS

5. Calculate the number of moles in: (a) 2.3 # of carbon (b) 0.014 g of Tin (c) a 5 Oz silver bracelet (d) a pound of table salt (e) a 350 Kg cast iron engine block (f) a gal. of water (8.3 #) (g) a ton of sand (SiO2) (h) 6.2 grams of blue vitriol (i) a pound of Epsom salts

Here for the first time we will be using DA method to change between mass and mols of a material. The conversion factor will be the formula weight of the material. There may be a little more DA to get the amount of material into units of grams, but that is just added to the main idea, that being that the formula weight is the way to get from mass to mols or from mols to mass of any material. Remember that the units of formula weight are grams per mol. Use the units in your calculations to keep your math straight.

Another way of thinking of the using the formula weight for a conversion factor is that for every material, the formula weight of it in grams is equal to a mol of that material.

The only real differences among these problems are the different formula weights of the materials and different ways to express the given amount of the material in grams so that they can be converted to mols.

Problem 5 f has an interesting part to it. The amount of material was given in volume rather than mass. An English volume, at that. The way shown here is via the English weight density of the water. There are several ways to do this, but I knew the number to make it quicker. The metric density of water is 1 g/cc, but getting the volume from gallons to cc's can be a pain. Try it yourself.

### PROBLEM #6, SET 1 - MOLS

6. Calculate the number of atoms in: (a) 100 g of Argon (b) 1.21 Kg aluminum foil (c) a 28 # lead brick (d) the E7 Kg of water in an olympic swimming pool (e) 7 Kg of hydrogen gas (f) a tonne of calcium nitrate

Now we can investigate the relationship between mols and number of molecules or atoms. You could call the units of Avogadro's Number atoms per mol or molecules per mol or just formulas per mol, depending upon how the material in question naturally comes. A mol of the element tin is Avogadro's number of atoms because elements come in atoms. A mol of water is Avogardo's number of molecules because water doesn't come any other way. A mol of blue vitriol, Cu(SO4)•5H2O, is Avogogadro's number of the whole formula, to include the water parts. Even though the formula comes apart into ions in solution and the water parts are not chemically attached, the entire group of atoms makes up a formula."

You can see that we have to calculate the number of UNITS of the material, whatever units it naturally comes in, and then consider the number of atoms in each unit of the material. (I have not given the raw answers in some of the problems above to save space.)

### PROBLEM #7, SET 1 - MOLS

7. What is the percentage composition of oxygen in each of the following materials: (a) CO (b) CO2 (c) (NO3)- (d) isopropyl alcohol C3H8O (e) calcium nitrate (f) blue vitriol Cu(SO4)•5H2O

Percentage is defined as: the target over the total times 100. Percentage composition is a common statistical treatment for a subset of a material within a larger material, for instance the percentage of sand in a concrete mixture or the percentage of males under twelve years old in the population of the United States populaion.

### PROBLEM #8, SET 1 - MOLS

8. What is the percentage composition of phosphate in each of the following materials: (a) phosphoric acid (b) sodium carbonate (c) ammonium phosphate (d) aluminum phosphate

### PROBLEM #9, SET 1 - MOLS

9. What is the percentage composition of sulfate in each of the following materials: (a) sulfuric acid (b) sodium sulfate (c) Epsom salts (d) aluminum sulfate