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QUESTION 1 Consider some unknown compound containing only copper and oxygen. In order to determine the empirical formula, a sample of the compound is decomposed into the elements copper and oxygen. The original sample had a mass of 0.6349 g prior to decomposition. After the reaction, 0.5073 g of pure copper solid was recovered. How many moles of copper were initially in the sample? As always, you should include a unit (mol). Use 63.55 g/mol as the molar mass of copper. .01000 mol Copper QUESTION 2 Since the original compound only contained copper and oxygen, once you extract and measure the amount of copper you can determine the amount of oxygen from the difference to the starting mass. In a 0.6349 g sample of the compound, if 0.5066 g of pure copper is extracted, how many moles of oxygen must have been in the compound? Use 16.00 g/mol as the molar mass of atomic oxygen. I .008019

QUESTION 1 Consider some unknown compound containing only copper and oxygen. In order to determine the empirical formula, a sample of the compound is decomposed into the elements copper and oxygen. The original sample had a mass of 0.6349 g prior to decomposition. After the reaction, 0.5073 g of pure copper solid was recovered. How many moles of copper were initially in the sample? As always, you should include a unit (mol). Use 63.55 g/mol as the molar mass of copper. .01000 mol Copper QUESTION 2 Since the original compound only contained copper and oxygen, once you extract and measure the amount of copper you can determine the amount of oxygen from the difference to the starting mass. In a 0.6349 g sample of the compound, if 0.5066 g of pure copper is extracted, how many moles of oxygen must have been in the compound? Use 16.00 g/mol as the molar mass of atomic oxygen. I .008019

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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QUESTION 1 Consider some unknown compound containing only copper and oxygen. In order to determine the empirical formula, a sample of the compound is decomposed into the elements copper and oxygen. The original sample had a mass of 0.6349 g prior to decomposition. After the reaction, 0.5073 g of pure copper solid was recovered. How many moles of copper were initially in the sample? As always, you should include a unit (mol). Use 63.55 g/mol as the molar mass of copper. .01000 mol Copper QUESTION 2 Since the original compound only contained copper and oxygen, once you extract and measure the amount of copper, you can determine the amount of oxygen from the difference to the starting mass. In a 0.6349 g sample of the compound, if 0.5066 g of pure copper is extracted, how many moles of oxygen must have been in the compound? Use 16.00 g/mol as the molar mass of atomic oxygen. .008019 QUESTION 3 In lab this week, your unknown copper-chloride compound will start out as a hydrate, which means it has a formula of CuxCly zH₂0. Your objective will be to calculate the ratio x:y:z by determining the mole amounts of each component Click Save and Submit to save and submit. Click Save All Answers to save all answers. F4 DII F5 ☀ F6 F7 PrtScn F8 Home F9 End FT
Transcribed Image Text:QUESTION 1 Consider some unknown compound containing only copper and oxygen. In order to determine the empirical formula, a sample of the compound is decomposed into the elements copper and oxygen. The original sample had a mass of 0.6349 g prior to decomposition. After the reaction, 0.5073 g of pure copper solid was recovered. How many moles of copper were initially in the sample? As always, you should include a unit (mol). Use 63.55 g/mol as the molar mass of copper. .01000 mol Copper QUESTION 2 Since the original compound only contained copper and oxygen, once you extract and measure the amount of copper, you can determine the amount of oxygen from the difference to the starting mass. In a 0.6349 g sample of the compound, if 0.5066 g of pure copper is extracted, how many moles of oxygen must have been in the compound? Use 16.00 g/mol as the molar mass of atomic oxygen. .008019 QUESTION 3 In lab this week, your unknown copper-chloride compound will start out as a hydrate, which means it has a formula of CuxCly zH₂0. Your objective will be to calculate the ratio x:y:z by determining the mole amounts of each component Click Save and Submit to save and submit. Click Save All Answers to save all answers. F4 DII F5 ☀ F6 F7 PrtScn F8 Home F9 End FT
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