Determining the emphirical formula of a compound

# Determining the emphirical formula of a compound -...

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Determining the Emphirical Formula of a Compound Abbey Blair 1/11/16 Period 5 Safety: In this lab we wore goggles as we handled two hazardous chemicals such as copper metal and sulfur. Sulfur is hazardous because when it is burned it produces toxic sulfur dioxide. Copper metal is considered non-hazardous but unpredictable reactions can always occur. Procedure: Page 30 Data and Observations: Mass of empty crucible + cover: 16.52g Mass of crucible + cover + copper: 17.13g Mass of crucible + cover + copper sulfide: 17.26g Calculations: 1. Find the mass of the copper used: 17.13g - 16.52g = 0.61g Cu 2. Find the mass of the sulfur that reacted: 17.26g - 17. 13g = .13g S 3. Calculate the number of moles of Cu used: .16Cu/63.546g/molCu = 0.009mol Cu 4. .13g S - 32.066 mol S = 0.0041 mol S 5. .0096/0.0041= 2.34 Cu 2.34 S1----> Cu 2 S 1 .0041/.0041= 1 Questions: 1. Write the emphirical formula of the copper sulfide based on your calculations from this experiment: Cu2S 2. Describe the appearance of the copper metal: It has a red-orange metallic luster.

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Describe the appearance of the sulfur: Sulfur has lemon yellow sintered microcrystals.
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