Lab Report Measuring Mass r6a5p

Collaku 1

Silvi Collaku Science Mr.ir Kellezi 14 Ocober 2015

Measuring mass: A means of counting Part One:Literature review During this unit, it was made known to us many interesting things of which we went deeper into. To understand what this unit is about, one must first apprehend several basic and their functions. Let us start from the beginning. Matter is something which is used everywhere especially in Chemistry and in this recent unit. Matter by definition is the physical material of the entire universe, everything that takes up space and that has mass. Everything is made of matter, the human body is made of matter, the chair that a person might sit on it made of matter, matter is all around us and should not be overlooked for without matter, the universe would not cease to exist. Another important term in this unit are moles. Moles are the most standard scienctific unit when it comes to measuring large quantites of small substances. The number of units in a mole is called Avogadro’s number (6.02x1023), which is the number of atoms resoluted to be in one mole. Then there is the molar mass. The molar mass is the mass of one mole and is presented in grams. In order to find the molar mass of e.g NaCl, one must first look at the Peridodic Table and find the element Na(sodium). Once you have found it you look at the atomic mass which, in this case is 23(rounded), now do the same for Cl(chlorine). After you have repeated the step for each of them you add both their atomic mass to find their molar mass. NaCl M= 23+ 35 M= 58 So the molar mass of NaCl is 58. It is crucial to know how to calculate the molar mass because it is something that is used habitually in Chemistry and without it one might not be able to solve certain chemical problems. The next thing is molar volume. Although molar volume is similar to molar mass, it is more commonly used when finding the volume of a gas. 1 mole of a gas occupies a specific volume at a certain temperature and pressure. It is 22.4 l/mol and remains so under any pressure or temperature.

Avogadro’s theory states that equal volumes of gases at the same temperature and pressure contain equal number of particles. Lastly there is percent compostition.The percent compostition is the number of grams of the element,divided by the mass in grams of the compound,then multiplied by 100%. To clculate you must find the molar mass of the compound and of the elements. Once you have found the percent

Collaku 2 compostition,you can also find the empirical formula of that compound. The empirical formula is a formula with the lowest number ratio of elements in a compound. Overall, when calculating all these things, it is very important to keep in mind The Law of Conservation of Mass. The law states that in any chemical reaction or physical change, mass is conserved. In other words,mass can neither be created nor destroyed. In a nutshell, knowing these things can really aid one when learning Chemistry, and can make it easier to calculate things, for if you know one, you know them all. Part Two: Problem statement, research question and Hypothesis. The problem for this unit was “Is it possible to calculate the atoms and moles of common compounds,objects and minerals?” In order to conduct an experiment to answer this problem, one must first have an hypothesis: If you measure the masses of compounds, objects, and/or minerals, then you will be able to calculate the particles that they contain. Above you will read the hypothesis for this experiment, but is it correct? Yes, it is correct because by measuring the mass of a compound, one can discover the different particles that are in the compound. However, it is not fully accurate and can be proven wrong until the conduction of the experiment. Part Three: Safety:    

Behave in a way that is consistant with a safe laboratory. Don’t chew gum, drink, or eat in the laboratory. Never taste a chemical in the laboratory. Wear the proper safety attire in the laboratory.

Materials:  Calcium fluoride - CaF2  Iron oxide - Fe2O3  Kevin - (C8H8)2  Sodium chloride - NaCl  Sucrose - C12H22O11  Sulfur - S  Dihydrogen monoxide - H2O  Silicon dioxide - SiO2  Calcium carbonate - CaCO3 Equipment:  plastic spoons  balance  plastic containers  glass slides

Procedure: 1. Measure the mass for each of the given compounds. 2. Find the molar mass for each of the given compounds. 3. After doing this find the number of moles for each of the compounds and all of the elements in said compounds. 4. Calculate the atoms of each element in all of the compounds.

Collaku 3 5. Complete the tables by writing down the results of the experiment. Data collection: In this experiment, several compounds and elements will be measured in order to determine their molar mass, amount of moles in each per teaspoon, moles in each, and the amount of atoms each contains. The compounds and elements being referred to are; sodium chloride, hydrogen monoxide, sucrose, silicon dioxide, calcium carbonate, a new compound called Kevin, sulfur, calcium fluoride, and iron oxide. During this experiment these exact elements will be measured in order to find their mass in mg, which, according to the hypothesis, will help discover their molar mass, their moles, the moles each contains, and the amount of atom in each. This data will be presented in three different tables, one for counting particles common substances, one for counting particles common materials, and one for counting particles in minerals. This data will help prove my hypothesis by discovering each compound/elements’ particles. Part Four:

Table 13.1

Counting Particles in Common Substances

Name Formula NaCl H2O

Molar mass

Moles in 1 teaspoon

sodium chloride

22,000mg

58 g/mols

0.379.3

hydrogen monoxide

2,000mg

18 g/mols

0.1

C12H22O11 sucrose

Table 13.2

Mass in mg

69,000mg

342 g/mols

.2.01

Counting Particles in Common Items

Moles of each element

Atoms of each element

0.379.3 moles Na

2.28x1023 atoms Na

0.379.3 moles Cl

2.28x1023 atoms Cl

0.1 moles H

0.602x1023 atoms H

0.1 moles O

0.602x1023 atoms O

.2.01 moles C

12.1002x1023 atoms C

.2.01 moles H

12.1002x1023 atoms H

.2.01 moles O

12.1002x1023 atoms O

Collaku 4

Name

Mass in mg

Molar mass

Moles in 1 sample

Moles of each element

Formula SiO2

silicon dioxide

15,000mg

60g/mols

0.250

0.250 moles Si 0.250 moles O

0.124,4 moles Ca CaCO3

calcium carbonate

27,000mg

217g/mols

0.124,4

0.124,4 moles C 0.124,4 moles O

CHCH2

Kevin C 6H 5

Table 13.3

10,000mg

212g/mols

n

Counting Particles in Minerals

0.0212

0.0212 moles C 0.0212 moles H

Atoms of each element 1.505x1023 atoms Si 1.505x1023 atoms O

0.748x1023 atoms Ca 0.748x1023 atoms C 0.748x1023 atoms O 0.127x1023 atoms C 0.127x1023 atoms H

Collaku 5

Formula

S

CaF2

Fe2O3

Name

Mass in mg

Molar mass

Sulfur

6,000mg

32 g/mol

calcium fluoride iron oxide

9,000mg

3,000mg

78 g/mol

86 g/mol

Moles

0,1875

0,1153

0,03488

Moles of each element

Atoms of each element

0,1875 moles S

1.128x1023 atoms S

0,1153 moles Ca

0.694 x1023 atoms Ca

0,1153 moles F

0.694 x1023 F

0,03488 moles Fe

3.0 x1023 atoms Fe

0,03488 moles O

3.0 x1023 atoms O

Part Five: I believe that the hypothesis for this experiment was correct because, after conducting the experiment, I was able to determine the different particles in each compound just as was hoped to. As shown in the tables above, the number of moles in a compound is equal to the number of moles in each element of that compound. I proved my hypothesis by calculating the mass of each substance out of three substances for each table. All my data is listed in the tables above. The next particle to be found was the molar mass, this must be done in order to discover just how many moles there is in the compound. This is how it is found: 1 mole = molar mass --------- --------------x moles = mass given Meaning that: x moles = 1 mole x mass given --------------------------molar mass Since I have the mass of each compound I still have to discover the moles if I want to calculate the numbers accuratly by using the formula. Because Avogadro’s number is perpetual, reluting in them have the same number of atoms as well as the same number of moles. This means that the number of moles in a compound is equivalent to that of the number of moles in the elements. However, I do not believe that the method used was entirely accurate. For example, for this experiment the entire class was divided into groups each measuring the same things, however, the results were not the same for every group. I believe that this error occcured because of the method that we used. It is possible that we did not measure everything correctly or that our equipment was broken. However, it is strange that all of the equipment in each qroup was broken. But I suppose that this occurred because each of the groups used different measurements for each compound/element.

So that the experiment conducted is more explicable, I have conducted anonther one exactly the same but with different substances.

Collaku 6 1. Design and carry out an experiment that will determine the number of atoms of calcium, carbon, and oxygen it takes to write your name on the chalkboard with a piece of chalk. Assume chalk is 100 percent calcium carbonate (CaCO3). The difference that resulted, you subtract by the atomic mass of CaCO 3. Atomic Mass Ca – 40g C – 12g O – 3x 16 = 48g _______________ (CaCO) = 100g/mol 40g - 35g = 5g 5g ------- = 0.05 moles 100g/mol

100% CaCO3 Ca  40% C  12% O  48%

0.05mol x 40% = 0.02 mol Ca 0.05mol x 12% = 0.006 mol C 0.05mol x 48% = 0.024 mol O

Works Cited "Chemistry, The Central Science 13th Ed - Brown (Pearson) Pdf." Torrent . Web. 19 Oct. 2015. . "Molar Volume of a Gas." Molar Volume of a Gas. Web. 19 Oct. 2015. . Information learned in class Papers handed out by the teacher