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

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 7CR

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