A 10.68 g sample of compound that contains only carbon, hydrogen, and oxygen was analyzed through combustion analysis and yielded 16.01 g of CO2 and 4.37 g of H2O. What is this compound's empirical formula? A) C4H13015 B) CH130 C) C3H403 D) C3H2O3
A 10.68 g sample of compound that contains only carbon, hydrogen, and oxygen was analyzed through combustion analysis and yielded 16.01 g of CO2 and 4.37 g of H2O. What is this compound's empirical formula? A) C4H13015 B) CH130 C) C3H403 D) C3H2O3
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 12 of 37**
A 10.68 g sample of a compound that contains only carbon, hydrogen, and oxygen was analyzed through combustion analysis and yielded 16.01 g of CO₂ and 4.37 g of H₂O. What is this compound's empirical formula?
- A) C₄H₁₃O₁₅
- B) CH₁₃O
- C) C₃H₄O₃
- D) C₃H₂O₃
This question requires determining the empirical formula of the compound based on the combustion products. The analysis involves converting the masses of CO₂ and H₂O to amounts of carbon, hydrogen, and oxygen present in the original compound. Then, those amounts are used to deduce the simplest whole-number mole ratio of the elements in the compound, which constitutes the empirical formula.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F81a44892-e725-436e-9c8e-21f599a0ba84%2F7c1f8739-6923-493b-9cf5-30bcf7de2637%2Fc7gxfbh.jpeg&w=3840&q=75)
Transcribed Image Text:**Question 12 of 37**
A 10.68 g sample of a compound that contains only carbon, hydrogen, and oxygen was analyzed through combustion analysis and yielded 16.01 g of CO₂ and 4.37 g of H₂O. What is this compound's empirical formula?
- A) C₄H₁₃O₁₅
- B) CH₁₃O
- C) C₃H₄O₃
- D) C₃H₂O₃
This question requires determining the empirical formula of the compound based on the combustion products. The analysis involves converting the masses of CO₂ and H₂O to amounts of carbon, hydrogen, and oxygen present in the original compound. Then, those amounts are used to deduce the simplest whole-number mole ratio of the elements in the compound, which constitutes the empirical formula.
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