10/19/2011 Akruti Patel Lab Report #4: Determination of a chemical formula: the empirical formula of Magnesium Oxide 1. Purpose: Determine the empirical formula of magnesium oxide from the percent composition (this can found using the Analytical Method and the Synthesis Method). 2. Introduction: In the late eighteenth century‚ combustion has been studied extensively. In fact‚ according to Steven and Susan Zumdahl‚ Antoine Lavoisier‚ a French Chemist‚ performed thousands of combustion experiments
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Observations/Qualitative Data: I have used my sense to observe that the magnesium is a solid that is bendable‚ is very light and its color is silver. After being put in a Crucible covered by a lid‚ under a Bunsen burner for a few minutes‚ it has lit up and turned red. After the experiment was over‚ the magnesium was turned into an ash/powdery state and its color became white/grey. Data collection and Processing (DCP): Quantitative Data: Weight in grams of the Magnesium before and after the experiment. Data table: The
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Chemistry Practical Report: Topic: Determining the Empirical Formula of Magnesium Oxide Patrick Doan 11 CHEM 11 26/9/08 Table of contents 1.0 Aim 1 2.0 Theory 2-3 3.0 Materials 4 4.0 Method 4 5.0 Results 4 - 5.1 Qualitative Observations 4 - 5.2 Example Calculations for each Calculated Value 5-7 -5.21 Experimental Values and Associated Errors 5-7 - 5.3 Accumulated Raw Data 8 - 5.4 Mean Experimental
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of Magnesium Oxide: Lab Report The objective of the experiment is to determine the empirical formula of Magnesium Oxide through a procedure of heating magnesium ribbon to react with oxygen to form a magnesium oxide compound with the correct ratio of atoms within each element; 1:1. Equipment: REFER TO EXPERIMENT SHEET Method: REFER TO EXPERIMENT SHEET Results: Object | Mass (g) | Crucible + Lid | 38.23 | Crucible + Lid + Magnesium | 38.57 | Crucible + Lid+ Magnesium Oxide | 38
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The Magnesium Oxide Lab In a compound the atoms of different elements are present in numbers whose ratio is usually an integer or a simple fraction. The simplest (or empirical) formula of the compound expresses that ratio. Simplest formulas are determined by establishing the mass of each element present in a sample of the compound. From those masses one finds the number of moles of each element present. The mole ratio is also the atom ratio in the compound and that ratio provides the subscripts
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The purpose of this lab was to find the empirical formula for magnesium oxide. To find this formula‚ a strip of Magnesium ribbon was burned in a crucible over a flame from a bunson burner. After the strip caught fire multiple times with the cover on‚ and 10 drops of distilled water were added‚ and the crucible was lightly heated. The crucible was then weighed and the mass recorded. Calculations were performed and the mole ratio of Mg to O was recorded. The results of other lab groups performing
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chemical properties of refractory of rotary kiln‚ it can be divided into alkaline‚ acidic and neutral refractories; 2. The chemical composition of refractory material of rotary kiln‚ it can be divided into silicon‚ aluminum‚ aluminum silicate‚ magnesium oxide‚ alumina‚ silicon carbide‚ carbon‚ etc. 3. According to the combination of rotary kiln refractory material‚ it can be divided into cement‚ chemical composition‚ condensing combination‚ etc. 4. During installation the refractory material
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of moles will be 13 moles of oxygen to 1 mole of lead. In the experiment‚ the students will find the empirical formula of a compound containing magnesium and oxygen. Based on prior knowledge‚ the student believes that the ratio of magnesium cations to oxygen anions will be one to one. The student also believes that the ratio of moles of magnesium to moles of oxygen will not be one to one. Materials and Equipment: Equipment: ● ● ● ● ● ● ● ● ● Crucible Crucible Tongs Clay Triangle Ring Stand w/ Clamps
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The Empirical Formula of Magnesium Oxide. Focus Question – Can the mass of magnesium combusted in excess oxygen be used to determine the empirical formula of magnesium oxide? Hypothesis – Combustion of Magnesium will generate data which can be used to calculate the EF of Magnesium Oxide Experimental Report: Data Collection and Processing Qualitative Observations: * The Magnesium burnt with a very bright flame. (as seen in figure 2 below) * White smoke was formed and some
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Aspect 1: Problem: What is the molar enthalpy of formation of magnesium oxide? Variables: Manipulated: None Responding: None Controlled: Isolation of calorimeter‚ concentrations of substances involved. Aspect 2: Background Information: Assumptions: Specific heat capacity of water‚ we assume that the acid has the same qualities as water including heat capacity‚ and we assume the enthalpy of formation for magnesium oxide from the data booklet for theoretical value. Hess’s Law:
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