MY Lap assignment

Theoretical and

actual yields of

Magnesium chloride

Name of the module: Chemistry

Assessment number: 1

Word count: 1700

Theoretical and actual yields of magnesium chloride

Aim:

The aim of the practical was to carry out the experiment by reacting magnesium with

hydrochloric acid and to calculate theoretical and actual yields of products based on

given amount of reactants.

Introduction:

One of the well-known laws in chemistry is the Law of Conservation of Mass

discovered by Russian scientist Mikhail Lomonosov in 1756 (APS News 2011) and

states that mass of the reactants is equal to the mass of products made in chemical

reactions. Therefore, the number of atoms used in the experiment will be the same as

the outcome of the reaction. This means that it is impossible to destroy or create an

atom during chemical experiment (Gorzynski-Smith 2013: 126-127).

Based on the law of conversation of mass, the reaction of magnesium with hydrochloric

acid to make magnesium chloride which is shown in the following chemical equation

as: Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g), theoretically shows that there are equal

number of atoms on both sides, so the mass of atoms will stay the same.

However, what can change in the reaction are the bonds between elements, so the

formation of new bonds or degradation may occur leading to creation of different types

of molecules (Gorzynski-Smith 2016: 134-135). Moreover, for reactants to form a new

compound the collision is necessary, so they must collide energetically between each

other in order to break and form bonds, which is known as collision theory. For

example, when a water molecule is made the hydrogen atom is burned and combined

with oxygen as shown in the chemical equation: 2H2(g) + O2(g) → 2H2O(l). This shows

that reactants, in this case 2H2 and O2, are equal to the products of this reaction, which

is 2H2O, because there are 4 hydrogen and 2 oxygen atoms in both sides of the

equation as shown on figure 1. Therefore, the total mass of reactants is equal to the mass of products as there was no gain or loss of any atom but only creation of covalent

bond to form a water molecule (McMurry, Fay and Robinson 2016: 70-71).

Figure 1. Chemical reaction between hydrogen and oxygen molecules to produce water (Online Chemistry Book n.d.).

In addition to, stoichiometry is the field in chemistry which revolves around quantitative

relationship between reactants and products, such as the actual and theoretical

percentage yields to determine how much of products were produced during chemical

reaction (Hein and Arena 2014: 169-181). The percentage yields are quite important

area in industry and all the companies spend much time and money to improve it. This

is because no matter what is produced, they want it in large quantities and as cheap

as it is possible, so therefore they are using percentage yields in order to estimate the

amount of product they can make and the cost of the production. In addition, it is used

to make sure that the synthesized reaction at every step progress in high yields

because if at any step will be low percentage yield, it will cause unnecessary waste of

reactants and money (Gorzynski-Smith 2016: 167).

In chemistry, to demonstrate the number of atoms of each element within a compound,

the empirical and molecular formulas can be used. The empirical formula shows the

simplest and smallest whole number ratio of each element within the molecule e.g.

glucose empirical formula is CH2O (Hein and Arena 2014 133-135). In order to find out

empirical formula three things are needed: the elements, which are combined with

each other; atomic mass of each element; and either the ratio percentage or mass in

the proportion they are combined (Marry, Fay and Robinson 2016 120-121).

Example of the Percent composition of glucose:

C – 40.00% (12.011u), H – 6.7% (1.008u), O – 53.3% (15.999u) (Hein and Arena 2014: 56)

Molar mass of glucose: (4 x 12.011) + (12 x 1.008) + (6x15.999) = 𝟏𝟏𝟏𝟏𝟏𝟏. 𝟏𝟏𝟏𝟏𝟏𝟏

𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁 𝑜𝑜𝑜𝑜 𝑁𝑁𝑜𝑜𝑚𝑚𝑁𝑁𝑚𝑚 𝑜𝑜𝑜𝑜 𝐶𝐶 = = 𝟏𝟏. 𝟏𝟏𝟏𝟏 𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎

𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁 𝑜𝑜𝑜𝑜 𝑁𝑁𝑜𝑜𝑚𝑚𝑁𝑁𝑚𝑚 𝑜𝑜𝑜𝑜 𝐻𝐻 = = 𝟏𝟏. 𝟏𝟏𝟏𝟏 𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎

𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁 𝑜𝑜𝑜𝑜 𝑁𝑁𝑜𝑜𝑚𝑚𝑁𝑁𝑚𝑚 𝑜𝑜𝑜𝑜 0 = = 𝟏𝟏. 𝟏𝟏𝟏𝟏 𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎

𝐷𝐷𝐷𝐷𝐷𝐷𝐷𝐷𝐷𝐷𝑁𝑁 𝑎𝑎𝑚𝑚𝑚𝑚 𝑡𝑡ℎ𝑁𝑁 𝑎𝑎𝑎𝑎𝑚𝑚𝑎𝑎𝑁𝑁𝑁𝑁𝑚𝑚 𝑁𝑁𝑏𝑏 𝑡𝑡ℎ𝑁𝑁 𝑚𝑚𝑁𝑁𝑎𝑎𝑚𝑚𝑚𝑚𝑁𝑁𝑚𝑚𝑡𝑡 𝑎𝑎𝑎𝑎𝑚𝑚𝑎𝑎𝑁𝑁𝑁𝑁: = 𝟏𝟏 = 𝟏𝟏. 𝟗𝟗𝟗𝟗 ≈ 𝟐𝟐 = 𝟏𝟏

Therefore, the empirical formula for glucose is CH2O.

At this time, the whole number ratios might be already obtained as in the example, so

the empirical formula can be written. But, if the numbers are decimals, all numbers

must be multiplied by the smallest number which will made them whole number, for

e.g. if A is 2,5 and B is 2, multiply it by 2, so the A will be equal 5 and B 4, which

represents the empirical formula as A5B4 (Marry, Fay and Robinson 2016: 120-121).

On the other hand, the molecular formula is used to represent the total number of

atoms within molecule but also arrangements of atoms for e.g. glucose molecular

formula is C6H12O6, which shows that within compound there are 6 carbons, 12

hydrogens and 6 oxygens. To determine the molecular formula, molar mass of the

compound and the empirical formula must be known, which then are applied to the

formula which looks following:

𝑀𝑀𝑜𝑜𝑚𝑚𝑎𝑎𝑁𝑁 𝑀𝑀𝑎𝑎𝑚𝑚𝑚𝑚 𝑎𝑎 = = 𝑎𝑎𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁 𝑜𝑜𝑜𝑜 𝑁𝑁𝑁𝑁𝑒𝑒𝐷𝐷𝑁𝑁𝐷𝐷𝑒𝑒𝑎𝑎𝑚𝑚 𝑜𝑜𝑁𝑁𝑜𝑜𝑁𝑁𝑁𝑁𝑚𝑚𝑎𝑎 𝑁𝑁𝑎𝑎𝐷𝐷𝑡𝑡𝑚𝑚

𝑀𝑀𝑎𝑎𝑚𝑚𝑚𝑚 𝑜𝑜𝑜𝑜 𝑁𝑁𝑁𝑁𝑒𝑒𝐷𝐷𝑁𝑁𝐷𝐷𝑒𝑒𝑎𝑎𝑚𝑚 𝑜𝑜𝑁𝑁𝑜𝑜𝑁𝑁𝑁𝑁𝑚𝑚𝑎𝑎

‘n’ is used to multiply the empirical formula in order to work out molecular formula, e.g.

for empirical formula of glucose the calculated n value is 6, the equation looks

following: (CH2O)6 = C6H12O6 the molecular formula for glucose (Hein and Arena 2014:

136).

Table 1. Examples of empirical and molecular formula of different compounds. Name of compound Empirical Formula Molecular Formula

Glucose CH2O C6H12O6 Methane CH4 CH4 Octane C4H9 C8H18 Caffeine C4H5N2O C8H10N4O2

Magnesium Chloride MgCl2 MgCl2 Ethyl Alcohol/Ethanol C2H6O C2H6O

Hydrogen peroxide HO H2O2

Sodium Phosphide Na3P Na3P

Moreover, the empirical formula for many compounds is usually identical to molecular

formula as shown in Table 1. This is because the formula cannot be simplified even

more as it already has low numbers, which cannot be divided, for e.g. MgCl2. On the

other hand, glucose molecule is made up of many atoms, so the molecular formula will

differ than empirical as the numbers can be divided, so C6H12O6 (molecular formula)

is simplified to give empirical formula of CH2O (Nivaldo 2014: 148).

Figure 2. Isomers and stereoisomers. However, in some occasion the empirical formula can be the same for different compounds such as for glucose, fructose and galactose. This is because these compounds are isomers and stereoisomers which means that they have identical formulas but different structures, so therefore even their molecular formula is the same (Mason et al 2017: 39).

Empirical formula of compound with mass of 0.662 containing 0.35g of Al and O.

Al = 0.35g

O = 0.662 - 0.350 = 0.312g 0.35g

𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁 𝑜𝑜𝑜𝑜 𝑁𝑁𝑜𝑜𝑚𝑚𝑁𝑁𝑚𝑚 𝑜𝑜𝑜𝑜 𝐴𝐴𝑚𝑚 = = 𝟎𝟎. 𝟎𝟎𝟏𝟏𝟐𝟐𝟗𝟗𝟎𝟎 𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎 26.982 (𝑁𝑁𝑜𝑜𝑚𝑚𝑎𝑎𝑁𝑁 𝑁𝑁𝑎𝑎𝑚𝑚𝑚𝑚 𝑜𝑜𝑜𝑜 𝐴𝐴𝑚𝑚)

0.312g 𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁 𝑜𝑜𝑜𝑜 𝑁𝑁𝑜𝑜𝑚𝑚𝑁𝑁𝑚𝑚 𝑜𝑜𝑜𝑜 𝑂𝑂 = = 𝟎𝟎. 𝟎𝟎𝟏𝟏𝟗𝟗𝟏𝟏𝟎𝟎 𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎

15.999 (molar mass of O)

= 𝟏𝟏 𝒙𝒙 𝟐𝟐 = 𝟐𝟐 = 𝟏𝟏. 𝟏𝟏 𝒙𝒙𝟐𝟐 = 𝟏𝟏

One of the answers is not a whole number, therefore it must be multiplied by 2 which

gives empirical formula of Al2O3.

Method:

At the start of the experiment, the measurements of some of the equipment and

sources were collected (shown in Table 3). Afterwards, the magnesium strip was

mixed with hydrochloric acid within the conical flask and by using syringe and the pipet;

the amount of hydrogen produced in the chemical reaction was calculated. Thirdly, the

homogenous mixture of Mg and HCl was moved to crucible, placed on the tripod and

gauze to be heated up using the Bunsen burner in order to make MgCl2 salt. Lastly,

the measurements of crucible were collected to find out how many salt was produced.

No list of reagents/equipments

Table 2. Risk assessment Hazards Risk Description Preventive Measures

Glass equipment

The glass during experiment may break. If it gets in contact with the skin, it may lead to the cut and bleeding but also may allow some bacteria to invade the wound.

In order to prevent it, the lab coat must be worn, to ensure most parts of the body are covered, as well as gloves to cover the hands and goggles to protect eyes. Also, making sure that the glass is not near the ledges to avoid it falling down and break.

Bunsen burner The flame form Bunsen burner is quite big, so therefore it may easily get in contact with hair or hands causing the skin or hair to burn.

To minimize the risk of getting in contact with the flame, hair should be tight up at all time. Furthermore, the safe flame can be used, so it will be clearly visible for everyone. Also, if the Bunsen burner is not in use, it should be turned off.

Hydrochloric Acid

Hydrochloric Acid is corrosive which means if it gets in contact with any part of the body it will burn the skin and can make damage to internal parts of the body.

To avoid contact with hydrochloric acid, the gloves, lab coat and goggles must be worn at all time in order to cover most parts of the body, therefore minimizing risk of contact with an acid.

No reference for risk assessment

Results:

Table 3. Data collected from the experiment Weight of Conical Flask 121.51 g

Weight of Conical Flask & Solution 135.85 g

Weight of Solution only 14.34 g

Weight of Magnesium Strip 0.02 g

Volume of gas produced 32 cm3

Conical flask after reaction 135.83 g

Weight of Crucible 28.63 g

Weight of Crucible & Salt 28.83g

Weight of Salt 0.20 g

Calculations to determine empirical formula for magnesium chloride:

Mg (molar mass) = 24.305 Cl2 (molar mass) = 2 x 35.453 = 70.906

24.305 + 70.906 = 95.211 (molar mass of MgCl2)

𝑃𝑃𝑁𝑁𝑁𝑁𝑁𝑁𝑒𝑒𝑁𝑁𝑎𝑎𝑡𝑡𝑎𝑎𝑃𝑃𝑁𝑁 𝑒𝑒𝑜𝑜𝑁𝑁𝑒𝑒𝑜𝑜𝑚𝑚𝐷𝐷𝑡𝑡𝐷𝐷𝑜𝑜𝑎𝑎 𝑜𝑜𝑜𝑜 𝑀𝑀𝑃𝑃 = 𝑥𝑥 100 = 𝟐𝟐𝟏𝟏. 𝟏𝟏𝟏𝟏%

𝑃𝑃𝑁𝑁𝑁𝑁𝑒𝑒𝑁𝑁𝑎𝑎𝑡𝑡𝑎𝑎𝑃𝑃𝑁𝑁 𝑒𝑒𝑜𝑜𝑁𝑁𝑒𝑒𝑜𝑜𝑚𝑚𝐷𝐷𝑡𝑡𝐷𝐷𝑜𝑜𝑎𝑎 𝑜𝑜𝑜𝑜 𝐶𝐶𝑚𝑚2 = 𝑥𝑥 100 = 𝟎𝟎𝟏𝟏. 𝟏𝟏𝟎𝟎%

𝑁𝑁𝑜𝑜. 𝑜𝑜𝑜𝑜 𝑁𝑁𝑜𝑜𝑚𝑚𝑁𝑁𝑚𝑚 𝑜𝑜𝑜𝑜 𝑀𝑀𝑃𝑃 = = 𝟏𝟏. 𝟎𝟎𝟏𝟏 𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎

𝑁𝑁𝑜𝑜. 𝑜𝑜𝑜𝑜 𝑁𝑁𝑜𝑜𝑚𝑚𝑁𝑁𝑚𝑚 𝑜𝑜𝑜𝑜 𝐶𝐶𝑚𝑚2 = = 𝟐𝟐. 𝟏𝟏 𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎

= 1 = 2

Therefore, the empirical formula for magnesium chloride is MgCl2. Since this formula

cannot be simplified, molecular formula for MgCl2 will be the same.

Calculations to determine percentage yields of products:

No. of moles of magnesium used = = 𝟖𝟖. 𝟐𝟐𝟏𝟏𝒙𝒙𝟏𝟏𝟎𝟎−𝟏𝟏

Balanced chemical equation for magnesium chloride:

Mg (s) + 2HCl (l) → MgCl2 (aq) + H2 (g)

No. of moles of H2 produced is equal 8.23x10-4, as the ratio between Mg and H2 is 1:1.

Percentage yield of MgCl2 and H2:

𝑁𝑁𝑜𝑜. 𝑜𝑜𝑜𝑜 𝑁𝑁𝑜𝑜𝑚𝑚𝑁𝑁𝑚𝑚 𝑜𝑜𝑜𝑜 𝑀𝑀𝑃𝑃𝐶𝐶𝑚𝑚2 𝑒𝑒𝑁𝑁𝑜𝑜𝐷𝐷𝑁𝑁𝑒𝑒𝑁𝑁𝐷𝐷 = = 𝟐𝟐. 𝟏𝟏𝟎𝟎𝒙𝒙𝟏𝟏𝟎𝟎−𝟏𝟏 𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎

2.10x10−3 𝑃𝑃𝑁𝑁𝑁𝑁𝑒𝑒𝑁𝑁𝑎𝑎𝑡𝑡𝑎𝑎𝑃𝑃𝑁𝑁 𝑜𝑜𝑜𝑜 𝑀𝑀𝑃𝑃𝐶𝐶𝑚𝑚2 produced = 8 .23x10−4 𝑥𝑥 100 = 𝟐𝟐𝟏𝟏𝟏𝟏%

32 cm3: 1000 = 0.032dm3 0.

𝑁𝑁𝑜𝑜. 𝑜𝑜𝑜𝑜 𝑁𝑁𝑜𝑜𝑚𝑚𝑁𝑁𝑚𝑚 𝑜𝑜𝑜𝑜 𝐻𝐻2 𝑒𝑒𝑁𝑁𝑜𝑜𝐷𝐷𝑁𝑁𝑒𝑒𝑁𝑁𝐷𝐷 == 𝟎𝟎. 𝟎𝟎𝟎𝟎𝟏𝟏𝟏𝟏 𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎𝒎

𝑃𝑃𝑁𝑁𝑁𝑁𝑒𝑒𝑁𝑁𝑎𝑎𝑡𝑡𝑎𝑎𝑃𝑃𝑁𝑁 𝑜𝑜𝑜𝑜 𝐻𝐻2 𝑁𝑁𝑜𝑜𝐷𝐷𝑁𝑁𝑒𝑒𝑁𝑁𝐷𝐷 = 𝑥𝑥 100 = 𝟏𝟏𝟏𝟏𝟐𝟐% 8.

Discussion:

The magnesium chloride is formed during single replacement reaction between Mg

(metal) and HCl (acid) which leads to the formation of an ionic bond between these

two elements (Gorzynski Smith 2016: 143-144). This is because Cl is in the seventh

group in periodic table, so it must gain only one electron to have 8 electrons in the

valence shell and become stable. On the other hand, Mg is in the second group in the

periodic table, so it must donate two electrons to become stable and achieve an octet.

Therefore, two chlorines are needed to create a compound. During redox reaction Mg

become an anion giving two electrons away (oxidation) and chlorines become cations

as they receive two electrons (reduction), one electron to each Cl element, in order to

form a magnesium chloride (MgCl2) salt (Nivaldo 2014: 250-251). Moreover, the

collision between particles is a key in chemical reaction as it allows to produce kinetic

energy, so the reactants can break and form bonds. In the Mg and HCl reaction, the

elevated temperature of the solution (exothermic reaction) and in the room speeded

up the movement of molecules, so therefore they collide with each other at increased

rate and at the same time accelerating the reaction. Moreover, more kinetic energy

was produced, so molecules were able to reach the activation energy which was

necessary for breaking bonds between HCl and formation of MgCl2 (Crowe and

Bradshaw 2014: 569-573).

According to the law of conservation of mass, when the experiment is complete, the

mass of the reactants supposed to be the same as the mass of products, so the

expected results would be 100% of each product. However, the results obtained after

experiment were much higher as 255% of MgCl2 and 162% of H2 were produced. One

of the reasons for this could be side reaction during an experiment. This is because

the experiment was done in the open space where multiple reactions occurred leaving

mixture of gasses in the air. Moreover, the conical flask was closed manually which

could have allowed some oxygen inside. Therefore, hydrogen produced during

reaction could react with oxygen forming covalent bond by sharing electrons between

them, forming water molecule (Smith 2013: 146). Furthermore, the formation of MgCl2

is exothermic reaction which means that the solution turned hot during experiment

(Lewis and Evans 2011: 216), so therefore the H2 reacting with oxygen would have

produced water in gaseous state, at the same time increasing the percentage yield of

H2 produced. In order to minimize this systematic error in future experiments, the

specialised equipment such as glovebox could be used. This is because this

equipment will allow to control pressure inside the vacuum (Yeada Group 2017), so

the atmospheric pressure can be minimized and allow to keep the solution in closed

compartment. Therefore, it will eliminate any additional reactants inside, so the

chances of hydrogen reacting with different elements will be minimal, making the

experiment more reliable and accurate.

Another reason for high percentage yield of products could be impurity. Since in the

experiment Mg was a limiting reactant (McMurry, Fay and Robinson 2016: 116-118),

a lot of HCl did not reacted.

Calculations to determine amount of HCl used:

No. of moles of magnesium used = = 𝟖𝟖. 𝟐𝟐𝟏𝟏𝒙𝒙𝟏𝟏𝟎𝟎−𝟏𝟏

Ratio between Mg and HCl is 1:2, so: 2 x 8.23x10-4 = 1.646x10-3

1.646x10-3 x (1.008 + 35.453) = 0.06g of HCl used for 0.02g of Mg

14.34 – 0.06 = 14.28 g of HCl did not reacted

Calculations of experimental formula for MgCl2:

Mass of Cl = 0.20 (mass of salt) – 0.02 (mass of magnesium strip) = 0.18g

𝑀𝑀𝑜𝑜𝑚𝑚𝑁𝑁𝑚𝑚 𝑜𝑜𝑜𝑜 𝑀𝑀𝑃𝑃 = = 𝟖𝟖. 𝟐𝟐𝟏𝟏𝒙𝒙𝟏𝟏𝟎𝟎−𝟏𝟏 𝑀𝑀𝑜𝑜𝑚𝑚𝑁𝑁𝑚𝑚 𝑜𝑜𝑜𝑜 𝐶𝐶𝑚𝑚 = = 𝟏𝟏. 𝟎𝟎𝟖𝟖𝒙𝒙𝟏𝟏𝟎𝟎−𝟏𝟏

8.22x10−4 𝑅𝑅𝑎𝑎𝑡𝑡𝐷𝐷𝑜𝑜 𝑁𝑁𝑁𝑁𝑡𝑡𝑎𝑎𝑁𝑁𝑁𝑁𝑎𝑎 𝑀𝑀𝑃𝑃 𝑎𝑎𝑎𝑎𝐷𝐷 𝐶𝐶𝑚𝑚 = 8 .22x10−4 = 𝟏𝟏 . 𝟏𝟏𝟖𝟖

≈ 𝟏𝟏 Therefore, experimental formula is MgCl6.

Furthermore, as already stated before the hydrogen could react with oxygen producing

water molecule, so it could get mixed with the HCl and dissolve an acid to produce

H3O+ + Cl- (hydronium and chloride ions) based on Arrhenius definition (Nivaldo 2014:

543). Therefore, the mixture of hydronium, chloride ions, excess of HCl and MgCl2 was

heated and most of it evaporated leaving crystal salt inside. However, because of the

high percentage yield of MgCl2, it is most likely that salt was impure which had an

impact on experimental formula of magnesium chloride. This means that human error

is another reason because product was not left for enough time to completely dry, so

the homogenous mixture of particles stated above could still be left inside, giving

incorrect results. In order to eliminate this error in the future, more time should be

allowed for the solution to fully dry. Therefore, all unwanted chemicals will have enough

time to evaporate and only desired product will remain in crucible, making the results

more accurate.

Conclusion:

The calculated percentage yields showed that when performing chemical reactions,

every little detail must be taken into consideration and every single step must be done

very accurately. This is because as looking back at the reaction of Mg and HCl a few

things, such as environment, human error or the equipment used had negative impact

on percentage yields of the product and those mistakes can be detrimental, especially

on the economy of industrial companies.

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