A 0.330 g of organic compound of unknown composition but containing carbon and hydrogen is burned with oxygen and produces 1.133 g of CO, and 0.185 g H20. Find the empirical formula of this compound. Moles of C in 1.133 g CO2 = 1.33 g CO2 x 1 mol CO2/44.01 g CO2× 1 mol C/1 mol CO2 = 0.02574 mol C Moles of H in 0.185 g H20 = 0.185 g H2O x 1 mol H20/18.02 g H20 x 2 mol H/1 mol H,O = 0.0205 mol H %3D Carrier gas Injector Detector Co.02574H0.0205 divide each by 0.0205 C1,26H, C5.04H4 C5H4 multiply each by 4 rounded to the closest integer number Column Flow/ pressure control Data system QUESTION O CHROMEDIA By carefully following the above example, answer this question: A mysterious compound sample, containing C, H and O, was collected at a crime scene. The sample was measured and subject to combustion analysis in which the sample of unknown composition was burned with oxygen gas. This combustion reaction produced only the two volatile products of CO2 and H2O. These two gaseous products were then separated and weighed by an automated instrument called a gas chromatograph. Using the data given to the right, determine the empirical formula of the sample. For your answer, type in the formula. DATA Mass of sample 0.450 g Mass of H,0 0.418 g Mass of CO2 1.023 g
A 0.330 g of organic compound of unknown composition but containing carbon and hydrogen is burned with oxygen and produces 1.133 g of CO, and 0.185 g H20. Find the empirical formula of this compound. Moles of C in 1.133 g CO2 = 1.33 g CO2 x 1 mol CO2/44.01 g CO2× 1 mol C/1 mol CO2 = 0.02574 mol C Moles of H in 0.185 g H20 = 0.185 g H2O x 1 mol H20/18.02 g H20 x 2 mol H/1 mol H,O = 0.0205 mol H %3D Carrier gas Injector Detector Co.02574H0.0205 divide each by 0.0205 C1,26H, C5.04H4 C5H4 multiply each by 4 rounded to the closest integer number Column Flow/ pressure control Data system QUESTION O CHROMEDIA By carefully following the above example, answer this question: A mysterious compound sample, containing C, H and O, was collected at a crime scene. The sample was measured and subject to combustion analysis in which the sample of unknown composition was burned with oxygen gas. This combustion reaction produced only the two volatile products of CO2 and H2O. These two gaseous products were then separated and weighed by an automated instrument called a gas chromatograph. Using the data given to the right, determine the empirical formula of the sample. For your answer, type in the formula. DATA Mass of sample 0.450 g Mass of H,0 0.418 g Mass of CO2 1.023 g
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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![### Determining the Empirical Formula of an Organic Compound
#### Example Calculation
Given:
A 0.330 g sample of an organic compound of unknown composition, containing only carbon and hydrogen, is burned with oxygen, producing the following:
- 1.133 g of CO₂
- 0.185 g of H₂O
**Step-by-Step Calculation:**
**1. Calculate moles of carbon in CO₂:**
\[ \text{Moles of C} = \frac{1.133 \, \text{g CO₂}}{44.01 \, \text{g/mol CO₂}} \times 1 \, \text{mol C} = 0.02574 \, \text{mol C} \]
**2. Calculate moles of hydrogen in H₂O:**
\[ \text{Moles of H} = \frac{0.185 \, \text{g H₂O}}{18.02 \, \text{g/mol H₂O}} \times 2 \, \text{mol H} = 0.0205 \, \text{mol H} \]
**3. Determine the empirical formula:**
\[ \text{C}_{0.02574}\text{H}_{0.0205} \quad \text{(Divide each by 0.0205)} \]
\[ \text{C}_{1.26}\text{H}_{1} \quad \text{(Multiply each by 4 and round to the nearest integer)} \]
\[ \text{Empirical Formula: C}_{5}\text{H}_{4} \]
#### Question
**By carefully following the above example, answer this question:**
A mysterious compound sample, containing C, H, and O, was collected at a crime scene. The sample was measured and subject to combustion analysis where it was burned with oxygen gas. This combustion produced only CO₂ and H₂O, separated and weighed by an automated instrument called a gas chromatograph. Using the data given to the right, determine the empirical formula of the sample.
**Data:**
| **Description** | **Mass** |
|-----------------|----------|
| Mass of sample | 0.450 g |
| Mass of H₂O | 0.418 g |
| Mass of CO₂ | 1.023 g |
**For your answer, type](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4167b07b-ab2c-42e3-ab89-9f12261de975%2Fe0c84b50-5eb8-4903-9d8f-60d2f5466c64%2Fts6lh86_processed.png&w=3840&q=75)
Transcribed Image Text:### Determining the Empirical Formula of an Organic Compound
#### Example Calculation
Given:
A 0.330 g sample of an organic compound of unknown composition, containing only carbon and hydrogen, is burned with oxygen, producing the following:
- 1.133 g of CO₂
- 0.185 g of H₂O
**Step-by-Step Calculation:**
**1. Calculate moles of carbon in CO₂:**
\[ \text{Moles of C} = \frac{1.133 \, \text{g CO₂}}{44.01 \, \text{g/mol CO₂}} \times 1 \, \text{mol C} = 0.02574 \, \text{mol C} \]
**2. Calculate moles of hydrogen in H₂O:**
\[ \text{Moles of H} = \frac{0.185 \, \text{g H₂O}}{18.02 \, \text{g/mol H₂O}} \times 2 \, \text{mol H} = 0.0205 \, \text{mol H} \]
**3. Determine the empirical formula:**
\[ \text{C}_{0.02574}\text{H}_{0.0205} \quad \text{(Divide each by 0.0205)} \]
\[ \text{C}_{1.26}\text{H}_{1} \quad \text{(Multiply each by 4 and round to the nearest integer)} \]
\[ \text{Empirical Formula: C}_{5}\text{H}_{4} \]
#### Question
**By carefully following the above example, answer this question:**
A mysterious compound sample, containing C, H, and O, was collected at a crime scene. The sample was measured and subject to combustion analysis where it was burned with oxygen gas. This combustion produced only CO₂ and H₂O, separated and weighed by an automated instrument called a gas chromatograph. Using the data given to the right, determine the empirical formula of the sample.
**Data:**
| **Description** | **Mass** |
|-----------------|----------|
| Mass of sample | 0.450 g |
| Mass of H₂O | 0.418 g |
| Mass of CO₂ | 1.023 g |
**For your answer, type
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