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A 0.4444 g of organic compound of unknown composition containing carbon, hydrogen and oxygen, is burned with oxygen, and produces 1.124 g of CO2 and 0.1822 g of H20. Calculate the mass of carbon, of hydrogen, and of oxygen that are contained in the organic compound. To obtain the exact answer, use the molar of C being equal to 12.01 g; the molar mass of H 1.010 g; the molar mass of O 16.00 g. In your answer, do not type in the unit gram, just type in the numbers that follow the rules of handling significant figures. Hint 1: Look up the example problem in the next, last question. Hint 2: Consider the law of mass conservation: the mass must be the same before and after a chemical reaction. The mass of carbon is g. The mass of hydrogen is g. The mass of oxygen is g.

A 0.4444 g of organic compound of unknown composition containing carbon, hydrogen and oxygen, is burned with oxygen, and produces 1.124 g of CO2 and 0.1822 g of H20. Calculate the mass of carbon, of hydrogen, and of oxygen that are contained in the organic compound. To obtain the exact answer, use the molar of C being equal to 12.01 g; the molar mass of H 1.010 g; the molar mass of O 16.00 g. In your answer, do not type in the unit gram, just type in the numbers that follow the rules of handling significant figures. Hint 1: Look up the example problem in the next, last question. Hint 2: Consider the law of mass conservation: the mass must be the same before and after a chemical reaction. The mass of carbon is g. The mass of hydrogen is g. The mass of oxygen is g.

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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### Problem Statement: A 0.4444 g of organic compound of unknown composition containing carbon, hydrogen, and oxygen, is burned with oxygen, and produces 1.124 g of CO2 and 0.1822 g of H2O. Calculate the mass of carbon, of hydrogen, and of oxygen that are contained in the organic compound. ### Given Data: - Mass of organic compound: 0.4444 g - Mass of CO2 produced: 1.124 g - Mass of H2O produced: 0.1822 g ### Constants: - Molar mass of Carbon (C): 12.01 g/mol - Molar mass of Hydrogen (H): 1.010 g/mol - Molar mass of Oxygen (O): 16.00 g/mol ### Instructions: To obtain the exact answer, use the molar masses provided. ### Answer Format: In your answer, do not type in the unit gram, just type in the numbers that follow the rules of handling significant figures. ### Hints: 1. Look up the example problem in the next, last question. 2. Consider the law of mass conservation: the mass must be the same before and after a chemical reaction. ### Calculations: - The mass of carbon is __________ g. - The mass of hydrogen is __________ g. - The mass of oxygen is __________ g.
Transcribed Image Text:### Problem Statement: A 0.4444 g of organic compound of unknown composition containing carbon, hydrogen, and oxygen, is burned with oxygen, and produces 1.124 g of CO2 and 0.1822 g of H2O. Calculate the mass of carbon, of hydrogen, and of oxygen that are contained in the organic compound. ### Given Data: - Mass of organic compound: 0.4444 g - Mass of CO2 produced: 1.124 g - Mass of H2O produced: 0.1822 g ### Constants: - Molar mass of Carbon (C): 12.01 g/mol - Molar mass of Hydrogen (H): 1.010 g/mol - Molar mass of Oxygen (O): 16.00 g/mol ### Instructions: To obtain the exact answer, use the molar masses provided. ### Answer Format: In your answer, do not type in the unit gram, just type in the numbers that follow the rules of handling significant figures. ### Hints: 1. Look up the example problem in the next, last question. 2. Consider the law of mass conservation: the mass must be the same before and after a chemical reaction. ### Calculations: - The mass of carbon is __________ g. - The mass of hydrogen is __________ g. - The mass of oxygen is __________ g.
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