the Empirical Formula of Silver Oxide Purpose: To find the percent composition and empirical formula of silver oxide can then be calculated‚ based on combining the ratios of silver and oxygen in the reaction. Hypothesis: Silver oxide decomposes to silver metal and oxygen when strongly heated. Heating Silver oxide causes the oxygen to be driven off‚ leaving only the silver metal behind. The total mass of the products of a chemical reaction must equal the mass of the reactants. Mass of silver oxide
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Buren 9/15/11 AP Chemistry Dr. Isotone Lab 1: Determination of the Empirical Formula of Silver Oxide Lab Objective: In this experiment‚ the percent composition and empirical formula of silver oxide will be determined. Silver oxide will be heated until it decomposes to silver metal and oxygen‚ and the percent calculation and empirical formula can be calculated based on combining the ratios of silver and oxygen in the reaction. Summary of Lab Procedure: 1. Set up
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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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Radha Shukla Determination of the Empirical Formula of Silver Oxide Will/Radha College Chemistry 9/12 – 9/13 9/17 The purpose of this lab is to use one of the ways to identify different compounds and be able to tell them apart. Based off of experimentation‚ the empirical formula of the given silver oxide will be determined. Materials: Chemicals: Silver Oxide‚ 0.5g Equipment: Balance‚ 0.001-g or 0.0001-g precision Bunsen Burner Clay pipestem triangle Crucible and cubicle lid‚ 15-
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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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DETERMINATION OF EMPIRICAL FORMULA OF MAGNESIUM OXIDE Objective: The objective of this lab is to experimentally determine the empirical formula of Magnesium Oxide. Equipment: • Ring Stand • 5 inch ring • wire gauze • Crucible and Crucible lid • Butane burner • Magnesium • Crucible tongs • Safety glasses • Gloves Experimental Procedure 1. Setup ring stand with five inch ring and triangle. 2. Obtain desired amount of Magnesium‚ a crucible with
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In this experiment‚ we have silver oxide and by using a bunsen burner‚ we will drive off all of the oxygen in the compound. We will do this by heating the silver oxide until the substance’s mass stays constant to know when all of the oxygen possible has been driven out. This process will occur through a series of heating and remassing. Silver oxide has many uses from batteries to military purposes. In a silver-zinc battery‚ silver oxide acts as the cathode and zinc as the anode. This battery is
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Empirical Formula of Magnesium Oxide Date: Aim: The aim of this experiment was to determine the empirical formula of magnesium oxide. Equipment: · Balance · Crucible and lid · Bunsen burner · Magnesium ribbon (0.2g) · Steel wool · Crucible tongs · Pipe clay triangle · Tripod Procedure: 1. Obtain a clean‚ dry crucible and lid‚ then heat them for approximately 5 minutes over a Bunsen burner 2. Clean the surface of a 20 cm strip of magnesium ribbon using steel wool 3. Coil
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Abstract In the Lab Determining the Empirical Formula of Magnesium Oxide‚ students set out to find if there is a true 1:1 ratio in the empirical formula of MgO. This was determined by burning the Magnesium until a white smoke started to protrude. This showed the reaction of Oxygen combining with Magnesium to form Magnesium Oxide. This was then measured again and turned out to be slightly heavier than the measurement before. This added weight is Oxygen‚ forming the combustion of Magnesium Oxide. The formula
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liquid it is essential that the 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
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