Name: J.T Empirical Formula 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
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Steven Leung 9/19/06 Lab Report The Empirical Formula of a Copper Oxide Purpose: To convert an unknown copper oxide to copper (Cu) metal using natural gas to provide a reducing environment as shown below: Cu O (s) + CH (g) ¨ Cu (s) + Co (g) + H O (g) From the mass difference between the unknown copper oxide and the Cu metal generated at the completion of the reaction and the molar mass of Cu and oxygen‚ the empirical formula of the original copper oxide can be calculated. Materials:
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Empirical Formula Lab Class: Chemistry 1405 Fall 2013 Aim: The aim of this Lab Exercise is to use the mass of a chemical and use that mass to find the amount of moles of the final product you can get using the empirical formula. Introduction: The empirical formula of a compound is the simplest whole-number ratio of the elements in the compound‚ which as you will discover‚ is a ratio of the moles of those elements. “Empirical” also means “experimentally determined”. In this experiment
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structure is derived. Firstly it is important to determine the percentage composition of elements to work out the empirical formula. The empirical formula was found to be C10H12O and the mass of the unknown was 148.09 m/z which when calculating the molecular weight of the empirical formula it did equal 148.09 g mol -1. This means that the empirical formula is also the molecular formula. As 12.01x10 carbons +1.008x12 hydrogens + 16= 148.09 09 g mol -1. From this knowledge the unknown molecule must
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Chemistry pre- IB Empirical Formula 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
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Lab of Determining an Empirical Formula B2 Honors 12/18/13 Abstract In this lab‚ to help better understand the concepts of gram atomic masses and empirical formulas‚ we found the gram atomic masses and empirical formula of a binary compound. The two compounds should form a definite whole number ratio by mass. This ratio will also help determine the subscripts of the elements in the empirical formula. Errors in this experiment can stem from measuring wrong or doing equations incorrectly.
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Glavin Wiechert Group Member: Victoria Coe Due Date: May 2‚ 2011 Teacher: Louth‚ Ellen Mary Class: Chemistry 11 Ad Introduction: An empirical formula of a chemical compound is the ratio of atoms in simplest wholenumber terms of each present element in the compound. For example‚ Glucose is C H O ; it’s empirical formula is CH O. 6 12 6 2 A hydrate is a compound that is chemically combined with water molecules. In contrast‚ an anhydrate does not contain water‚ and has had all of its water removed
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What is the empirical formula of a compound that contains 75% Ag and 25% Cl by mass? AGCL Calculate the approximate number of molecules in a drop of water with a mass of 0.10 g. 3 x 1021 molecules What is the percentage composition of CaSO4? 29.44% Ca‚ 23.55% S‚ 47.01% O What mass of calcium bromide is needed to prepare 150.0 mL of a 3.50 M solution? (Assume that the molecular weight of CaBr2 is 200.618 g/mol) 105 g Nitrous oxide (N2O)‚ or laughing gas‚ is commonly used as an anesthetic
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Experiment 5 Determination of Empirical Formulas of Hydrate and Oxide Compounds Room #216 Locker# 1137 Date of Experiment: May 11‚ 2014 Date of Submission: May 16‚ 2014 Purpose: To determine the identity of an unknown hydrated salt calculating the percent water loss after heating and also to determine the empirical formula of magnesium oxide. Results: Table 1: Determination of the mass of waters of hydration of an unknown hydrated compound. Hydrated Compound code: C-14 Mass
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Empirical Formula of a Compound * Purpose: To determine the empirical formula of Magnesium Chloride. * Data 1. Mass of evaporating dish = 45.08g 2. Mass of evaporating dish and Magnesium = 45.17g 3. Mass of Magnesium: { 2 } – { 1 } = 0.09 4. Mass of evaporating dish and Magnesium Chloride First weighing = 45.48g (After heating and cooling) second weighing = 45.49g 5. Mass of Magnesium Chloride: { 4} – { 1 } = 0.41g
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