...The Empirical formula of an oxide Lubna Abdulkhaleiq Oct/8/2015 Introduction: The purpose of this experiment is to determine the empirical formula of magnesium oxide from the results that you obtain by burning Magnesium. We can calculate the empirical formula by combining the masses of magnesium and oxygen. Before combining the Mg with oxygen we will weigh it and we will also weigh the product of the reaction, Magnesium Oxide. If magnesium is heated in open air, its reaction with oxygen is fast. We can slow down the reaction by limiting the supply of oxygen that reaches the magnesium; we do that by putting a cover on the crucible that contains the magnesium sample. magnesium + oxygen → magnesium oxide (a) 2Mg(s) + O2(g)⇒ 2MgO(s) magnesium + nitrogen →...
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...Determining the Empirical Formula of Magnesium Oxide Lab Purpose The purpose of this lab was to determine the percent composition and empirical formula of magnesium oxide. Hypothesis If a strip of pure magnesium metal reacts with oxygen in the air to create magnesium oxide, then the molecular formula will be MgO. The percent composition for magnesium oxide would be 60.31% magnesium and 39.69% oxygen. Apparatus Refer to attached sheet Procedure Refer to McGraw-Hill Ryerson Chemistry 11, page 212-213. 4. The mass of the empty crucible and lid was recorded. The strip of cleaned magnesium was added to the crucible. The mass of the crucible, lid and magnesium was recorded. 10. The substance remained in the crucible, above the flame for an extra five minutes on high heat, after the water had evaporated completely. Results Mass of clean, empty crucible and lid | 26.73g | Mass of crucible, lid, and magnesium | 26.87g | Mass of crucible and magnesium oxide | 26.95g | Analysis 1. a) We used 0.14 g of magnesium in the reaction. b) 0.22 g of magnesium oxide was produced. c) 0.08 g of oxygen reacted with the magnesium (0.22 g – 0.14 g = 0.08 g). d) Refer to “Determining the Empirical Formula of Magnesium Oxide Lab Solutions” sheet e) Element | % | m (g) | M (g/mol) | n (m÷M) | ÷ by | Ratio | Magnesium | 63.63 | 63.63 | 24.31 | 2.617441382 | 2.273125 | 1 | Oxygen | 36.37 | 36.37 | 16.00 | 2.273125 | 2.273125 | 1 | Since the ratio is 1:1,...
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...1. Give an everyday example that illustrates the difference between acceleration and velocity. Give an example of uniform and accelerated motion. An everyday example of the difference between acceleration and uniform motion would be for acceleration driving a car down a long straight road, the speedometer is not moving, the needle is on 40 mph, your moving at a constant speed, but the needle isn’t stationary on the speedometer scale because maybe your foot is either on the gas or brake and your speed is changing and your are accelerating. An example of uniform and accelerated motion would be a driving are car down a highway, accelerating to get to the speed limit which is 75 and uniform motion would be a car is cruising at 75 miles at that constant speed. 2. What determines the difference between scientific knowledge and non-scientific knowledge? What determines the different between scientific knowledge and non-scientific knowledge is that scientific knowledge is based on a body of techniques for investigating phenomena, acquiring new knowledge and integrating previous knowledge consisting of the data collected through observation, experimentation, and formulation and testing the hypothesis, basically using the scientific method to perform the results. Scientific knowledge is the knowledge that has been gained from analyzing evidence. Non-scientific knowledge is the gathering of information by people or institutions that do know use the scientific method. 3. Why do...
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...CuSO(Copper Sulfate) Dependent : Mass of curcible and magnesium; mass of curcible and magnesium oxide Control : Same mass of empty curcible, sama mass of magnesium before burned Materials Name of compound | Quantity | Hydrated cooper(II) sulfate (CuSO) | 1 | Bunsen Burner | 1 | Tripos stand | 1 | Pipeclay triangle | 1 | Crubicle | 1 | Pair of tongs | 1 | Electronic balencing | 1 | Sand paper | 3 | Procedures 1). Clean up the crucible until there’s nothing in it. 2). Weight an empty crucible. 3). Crush the CuSO until it become powder. 4). Measure the magnesium (CuSO) about 2 g. 5). Put it in the empty crucible. 6). Heat it until 5 minutes and another 5 minutes until the weight of crucible +magnesium after each minutes become constant. 7) Repeat step 3 – 6 for the second trial. Data Collection After Burned and the mass is constant. Trial | Mass of Crucible + Magnesium Oxide (g) | 1 | 55,19 g | 2 | 54,57 g | ∑Mass | 54,88 g | Trial | Mass of Crucible + Magnesium (g) | 1 | 54,19 g | 2 | 53,78 g | ∑Mass | 53,99 g | Results Mass of empty crucible = 52,38 g (A) Mass of crucible + Magnesium = 53,99 g (B) Mass of crucible + magnesium oxide = 54,88 g (C) Calculations Mass of magnesium used = (B) - (A) = 53,99-52,38 = 1,61 g Mass of magnesium oxide formed = (C) - (A) =...
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...Title of the experiment : EMPIRICAL FORMULA OF MAGNESIUM OXIDE Course : Experiment Number : 3 Instructor Name : Date : 17 June 2014 Objectives After carrying out the experiment, we are able to: 1. Determine the empirical formula for magnesium oxide 2. Gain practical experience in developing techniques using crucible Procedure 1. Heated a clean, dry porcelain crucible with cover on a clay triangle (supported on a ring stand), using a direct flame, for about 5 minutes. 2. Turned off the burner; allowed the crucible and covered to cool. Weighed the crucible and it covered on a balance. 3. Cut a 5-cm strip of magnesium ribbon, and removed the oxide layer by using sand paper. 4. After that, rolled the metal into flat coil. Placed the coil of magnesium in the crucible so that it lied flat against the bottom. Reweighed the crucible, cover and magnesium metal. NOTE: Don’t coil it so tightly that it will be difficult for magnesium to react completely. 5. Returned the crucible to the clay triangle. With the cover on, fired the crucible to red heat. Every few minutes, lifted crucible cover with a tong to see if the magnesium had started to burn and also to leave some air enter the crucible to make the experiment more efficient. 6. When the magnesium sparked and began to smoke, immediately removed the burner and placed the cover on the crucible using crucible tongs. ...
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...Determining the enthalpy of combustion of Magnesium Om Vora Ms. Mohoruk Lab Partner: Ujjwal Nambiar 4/25/16 IB HL Chemistry 11 Purpose: The purpose of this lab is to determine the molar enthalpy of combustion of Mg using Hess Law by manipulating three formulas, two of which will be found through the experiment and one value is already given. Materials: Refer to lab handout on the front of the page as no changes were made. Procedure: Refer to lab handout on the front of the page as no changes were made. Qualitative results: • Bubbles and vapor is released during the reaction of both Mg and MgO. • Solutions in the calorimeter got really hot after the mixing the two. Sign of exothermic reaction. • Small residue of...
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...1) Look up the chemical/health hazards for sulfur!. Main Routes of Exposure: Inhalation. • Inhalation: VERY TOXIC, can cause death. Can cause severe irritation of the nose and throat. At high concentrations: can cause life-threatening accumulation of fluid in the lungs (pulmonary edema). Symptoms may include coughing, shortness of breath, difficult breathing and tightness in the chest. A single exposure to a high concentration can cause a long-lasting condition like asthma. If this occurs, many things like other chemicals or cold temperatures can easily irritate the airways. Symptoms may include shortness of breath, tightness in the chest and wheezing. {Reactive Airways Dysfunction Syndrome (RADS)}. • Skin Contact: CORROSIVE. The gas irritates or burns the skin. Permanent scarring can result. Direct contact with the liquefied gas can chill or freeze the skin (frostbite). Symptoms of mild frostbite include numbness, prickling and itching. Symptoms of more severe frostbite include a burning sensation and stiffness. The skin may become waxy white or yellow. Blistering, tissue death and infection may develop in severe cases. • Eye Contact: CORROSIVE. The gas irritates or burns the eyes. Permanent damage including blindness can result. Direct contact with the liquefied gas can freeze the eye. Permanent eye damage or blindness can result. • Ingestion: Not a relevant route of exposure (gas). • Effects of Long-Term (Chronic) Exposure: May harm the respiratory system. Can irritate...
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...Lab Report By: Steven Setya 11B Hess’s Law: Determine Heat Formation of Magnesium Oxide Aim: To find Temperature difference/forming between MgO metal and Mg metal Hypothesis: My hypothesis is if Magnesium oxide has a heat formation due to the reaction with HCl, then Magnesium Metal will have a greater temperature difference. Variables: Independent: Amount of HCl Dependent: Temperature increase Controlled: Amount of Mg metal and MgO metal Manipulation Variable: The independent variable is the amount of HCl being reacted with Magnesium Metal and Magnesium Oxide. The more the amount of HCl the faster is the reaction and we can see the amount of heat change produced from the reaction. While the Dependent is the temperature increase during the reaction from the original room temperature of the solution. When Mg or MgO is reacted with HCl, reaction occurs and temperature increase will be there. What I control is the amount of Mg and MgO that will be reacted with HCl. If there is too much the reaction won’t be a fine reaction nor vice versa. Materials: 1 Bottle with hole in lid Beaker with 100 ml of 1 mol of HCl 0.10-0.15 grams of Magnesium 0.3-0.5 grams of Magnesium Oxide 1 Stopwatch 1 Thermometer (in Celcius) 1 Big Beeker with A lot of Cotton 2 10 ml Beeker Procedure: Experiment 1: 1. Take 0.15 grams of Magnesium Metal 2. Weigh the bottle and lid 3. Add 50ml of HCl to bottle and record new mass 4. Measure the temperature of HCl inside...
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...Acids dissociate to different extents in aqueous solution. Acids that dissociate to a large extent are strong electrolytes and strong acids. In contrast, acids that dissociate only to a small extent are weak acids and weak electrolytes In a similar manner, bases can be strong or weak depending on the extent to which they dissociate and produce OH– ions in solution. Most metal hydroxides are strong electrolytes and strong bases. Ammonia, NH3, is a weak electrolyte and weak base. o BASES eg oxides and hydroxides are substances that react and neutralise acids to form salts and water. Bases which are soluble in water are called alkalis. Acids Some common acids are listed below: Name Hydrochloric acid Sulphuric acid Nitric acid Ethanoic (acetic) acid Methanoic (formic) acid Citric Acid Formula HCl H2SO4 HNO3 CH3COOH HCOOH C6H8O7 Strong/Weak Strong Strong Strong Weak Weak Weak Where is it found? The stomach, in the lab. Acid rain, car batteries, the lab. Acid rain, in the lab. Vinegar Ant & nettle stings, descalers Citrus fruits Acids taste sour (e.g....
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...PHYSICAL PROPERTIES OF THE PERIOD 3 OXIDES These pages explain the relationship between the physical properties of the oxides of Period 3 elements (sodium to chlorine) and their structures. Argon is obviously omitted because it doesn't form an oxide. A quick summary of the trends The oxides The oxides we'll be looking at are: |Na2O |MgO |Al2O3 |SiO2 |P4O10 |SO3 |Cl2O7 | | | | | |P4O6 |SO2 |Cl2O | Those oxides in the top row are known as the highest oxides of the various elements. These are the oxides where the Period 3 elements are in their highest oxidation states. In these oxides, all the outer electrons in the Period 3 element are being involved in the bonding - from just the one with sodium, to all seven of chlorine's outer electrons. The structures The trend in structure is from the metallic oxides containing giant structures of ions on the left of the period via a giant covalent oxide (silicon dioxide) in the middle to molecular oxides on the right. Melting and boiling points The giant structures (the metal oxides and silicon dioxide) will have high melting and boiling points because a lot of energy is needed to break the strong bonds (ionic or covalent) operating in three dimensions. The oxides of phosphorus, sulphur and chlorine consist of individual molecules - some small and simple; others polymeric. The attractive forces between these molecules...
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...molecules together. There are many tests that can be performed to determine whether a molecule contains covalent or ionic bonds, and three of these tests will be utilized in this lab. The compounds will be tested for their solubility and conductivity in water, and their melting points will also be determined. Covalent compounds usually do not conduct electricity in water and have relatively low melting points. Ionic compounds are usually conductive in water and have very high melting points. Using data collected from these tests, bonds can be classified as covalent or ionic. Guiding Questions: Please answer the following questions before beginning the lab. 1. A compound has a melting point of 92 oC, does not dissolve in water, and does not conduct electricity in water. What type of compound is this? 2. A compound has a very high melting point, does dissolve in water, and conducts electricity in water. What type of compound is this? Equipment/Materials: Acetylsalicylic acid Capillary tubes Calcium carbonate Conductivity apparatus Deionized water Dextrose Digital Thermometer Disposable pipet Dropping Tube Magnesium sulfate Mel-Temps Naphthalene Scoopula Sodium chloride Stirring rod Urea Wash bottle of DI water Well plate Zinc oxide Safety: Goggles should be worn in the lab. The parts on the top of the Mel-Temp are HOT while it is...
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...During the experiment we encountered various problems. While weighing the magnesium, some of the strips fell and other strips fell off, therefore we had to weigh it again. When we did the first reaction, the final temperature of the reaction rose to only about 65C due to the fan and air conditioning in the area that we were working in. We consulted with the instructor, and he told us that the final temperature had to be at least 70C. We moved to another area where the fan was not blowing directly at us, and we did the first reaction again, finally obtaining the desired temperature. The next problems we encountered were in the calculations of the enthalpy for the reaction: Mg(s) + 1/2O2(g) MgO(s) At first, we forgot to change the enthalpies from the reactions that we produced to kilo Joules. Then, we consulted the instructor with our final answer, he said that we had to divide the enthalpies we found from the reactions that we produced by .05 mol, in order to calculate it with the other enthalpies, because the unit for enthalpy is kJ/mol. Theoretical Value: Mg(s) + 1/2O2(g) MgO(s) H = -601.8 kJ Experimental Value: Mg(s) + 1/2O2(g) MgO(s) H = -578.4 kJ Our experimental value is -23.4 kJ more than the theoretical value. Compared to the theoretical value, our percent error is: Percent Error: 578.4 kJ - 601.8 kJ x 100 % 601.8 kJ ...
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...We recently did two labs where we were given the task of observing single-replacement and double-replacement reactions. This paper has background information on the different types of chemical reactions, as well as the chemistry behind the two reactions we observed in lab. A chemical reaction is a process that is characterized by a chemical change in which the reactants (starting products) are different from the products. Chemical reactions involve the breaking of old bonds and the formation of new bonds. They can result in the formation of precipitates, changes in color, production or absorption of heat, or formation of gas bubbles. Chemical reactions can be placed in the following five categories: (i) synthesis (ii) decomposition...
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...dry) has the reddish-brown flaky character we associate with rust. Although the reaction that produces Fe(OH)2 is technically an equilibrium process (all electrochemical processes are) the value of Kc is very large (>1099 at 298 K) and left unchecked it will go to completion. But the rate is relatively slow under normal atmospheric conditions and so it is still possible to manipulate the equilibrium somewhat by changing appropriate factors. The rates of corrosion reactions--and presumably their mechanisms--vary widely. Factors which influence the progress of the net reaction in the first step of the oxidation of iron may have an effect on the overall rate. The nature of the oxide product is also very important in affecting the extent of the corrosion. For example, aluminum is a very active metal, but its oxide, Al2O3, is very dense and forms a thin protective layer on the metal which discourages further corrosion. In contrast, iron rust (hydrated forms of Fe2O3 such as reddish-brown Fe(OH)3) is typically flaky and easily crumbles off to continually expose fresh metal for reaction. Although the mechanism for corrosion is not always well understood, it is clear how to prevent it. The surface of the metal must be protected from contact with oxygen. Paints, oils and other coatings are often used for this purpose. But it is...
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...Coordinator : Dr Chee Swee Yong Lecturers : Ms Chang Chew Cheen, Dr Chee Swee Yong, Dr Lim Tuck Meng, Dr Sim Yoke Leng |Lab group |Lab A |Lab B | |Venue |D012A |D012B | |Monday @ 9.00 am – 11.30 am |P5 |P1 | |Monday @ 3.00 pm – 5.30 pm |P2 |P3 | |Wednesday @ 9.00 am – 11.30 am |P3 |P4 | |Wednesday @ 3.00 pm – 5.30 pm |P1 |P2 | |Thursday @ 3.00 pm – 5.30 pm |P4 |P5 | |Week |Experiment |Lab group |Lecturer | |1 |Briefing by HoD |Lab A/ Lab B |Dr Sim KM | | |Expt 1: Investigating the properties of Period 3 oxides |Lab A |Dr Chee SY | | | | | ...
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