Sample grams of a hydrocarbon, CxHy, were burned in a combustion analysis ap 5 of CO2 and 8.973 grams of H₂O were produced. e experiment, the molar mass of the compound was found to be 86.18 g e empirical formula and the molecular formula of the hydrocarbon. nter the elements in the order presented in the question. mpirical formula =
Sample grams of a hydrocarbon, CxHy, were burned in a combustion analysis ap 5 of CO2 and 8.973 grams of H₂O were produced. e experiment, the molar mass of the compound was found to be 86.18 g e empirical formula and the molecular formula of the hydrocarbon. nter the elements in the order presented in the question. mpirical formula =
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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![### Combustion Analysis of a Hydrocarbon
When 6.130 grams of a hydrocarbon, \( C_xH_y \), were burned in a combustion analysis apparatus, 18.78 grams of \( CO_2 \) and 8.973 grams of \( H_2O \) were produced.
In a separate experiment, the molar mass of the compound was found to be 86.18 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
#### Explanation of Graph (Diagram)
The diagram shows a combustion analysis apparatus. The apparatus includes:
- **Furnace**: Where the sample is burned in the presence of \( O_2 \).
- **CO_2 Absorber**: A container that absorbs the \( CO_2 \) produced.
- **H_2O Absorber**: A container that absorbs the \( H_2O \) produced.
#### Calculations
To determine the empirical formula and the molecular formula, follow these steps:
1. **Find the number of moles of carbon and hydrogen**:
- From the mass of \( CO_2 \): Obtain the moles of carbon.
- From the mass of \( H_2O \): Obtain the moles of hydrogen.
2. **Determine the simplest whole number ratio of the elements**:
- Use the moles calculated in the previous step to find the ratio.
3. **Calculate the empirical formula**:
- Convert the ratio into the simplest whole numbers.
4. **Find the molecular formula**:
- Use the molar mass to find the molecular formula based on the empirical formula.
#### Input Fields
Enter the elements in the order presented in the question.
Environmental formula = [ ]
Molecular formula = [ ]
Once all fields have been filled, click on the "Check & Submit Answer" button.
For more details on the process, you can click the "Show Approach" button to see the detailed steps.
**Check & Submit Answer**
**Show Approach**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4126b89b-6ee3-437f-8fcf-aa0e90855818%2Fc616343e-ab6d-41b7-91b7-316ca10d76b4%2F3dx4815_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Combustion Analysis of a Hydrocarbon
When 6.130 grams of a hydrocarbon, \( C_xH_y \), were burned in a combustion analysis apparatus, 18.78 grams of \( CO_2 \) and 8.973 grams of \( H_2O \) were produced.
In a separate experiment, the molar mass of the compound was found to be 86.18 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
#### Explanation of Graph (Diagram)
The diagram shows a combustion analysis apparatus. The apparatus includes:
- **Furnace**: Where the sample is burned in the presence of \( O_2 \).
- **CO_2 Absorber**: A container that absorbs the \( CO_2 \) produced.
- **H_2O Absorber**: A container that absorbs the \( H_2O \) produced.
#### Calculations
To determine the empirical formula and the molecular formula, follow these steps:
1. **Find the number of moles of carbon and hydrogen**:
- From the mass of \( CO_2 \): Obtain the moles of carbon.
- From the mass of \( H_2O \): Obtain the moles of hydrogen.
2. **Determine the simplest whole number ratio of the elements**:
- Use the moles calculated in the previous step to find the ratio.
3. **Calculate the empirical formula**:
- Convert the ratio into the simplest whole numbers.
4. **Find the molecular formula**:
- Use the molar mass to find the molecular formula based on the empirical formula.
#### Input Fields
Enter the elements in the order presented in the question.
Environmental formula = [ ]
Molecular formula = [ ]
Once all fields have been filled, click on the "Check & Submit Answer" button.
For more details on the process, you can click the "Show Approach" button to see the detailed steps.
**Check & Submit Answer**
**Show Approach**
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