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Here are some additional combustion analysis problems to practice: 1. A compound containing only carbon and hydrogen weighing 0.822 g was burned in oxygen to give 2.01 g of CO, and 0.827 g of H₂O. What is the empirical formula for the compound? 0.822 g CH 2. When 0.684 g of a compound containing only C, H, and O was burned in oxygen, 1.312 g of CO, and 0.805 g of H₂O were obtained. Determine the empirical formula of the compound.

Here are some additional combustion analysis problems to practice: 1. A compound containing only carbon and hydrogen weighing 0.822 g was burned in oxygen to give 2.01 g of CO, and 0.827 g of H₂O. What is the empirical formula for the compound? 0.822 g CH 2. When 0.684 g of a compound containing only C, H, and O was burned in oxygen, 1.312 g of CO, and 0.805 g of H₂O were obtained. Determine the empirical formula of the compound.

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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Here are some additional combustion analysis problems to practice: 1. A compound containing only carbon and hydrogen weighing 0.822 g was burned in oxygen to give 2.01 g of CO, and 0.827 g of H₂O. What is the empirical formula for the compound? 0.822 g CH 2. When 0.684 g of a compound containing only C, H, and O was burned in oxygen, 1.312 g of CO, and 0.805 g of H₂O were obtained. Determine the empirical formula of the compound.
Transcribed Image Text:Here are some additional combustion analysis problems to practice: 1. A compound containing only carbon and hydrogen weighing 0.822 g was burned in oxygen to give 2.01 g of CO, and 0.827 g of H₂O. What is the empirical formula for the compound? 0.822 g CH 2. When 0.684 g of a compound containing only C, H, and O was burned in oxygen, 1.312 g of CO, and 0.805 g of H₂O were obtained. Determine the empirical formula of the compound.
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