### Determining Empirical and Molecular Formulas of a CompoundAn unknown compound has the formula \( C_xH_yO_z \). You burn 0.2072 g of the compound and isolate 0.5059 g of \( CO_2 \) and 0.2071 g of \( H_2O \). What is the empirical formula of the compound? If the molar mass is 72.1 g/mol, what is the molecular formula?**Problem:** (Enter the elements in the order: C, H, O.)| Empirical formula: | [---Text Box for Answer---] || Molecular formula: | [---Text Box for Answer---] |In this problem, the goal is to find both the empirical and molecular formulas of the unknown compound. Let's break down the steps necessary to solve this problem.#### Step-by-Step Method:1. **Determine the amount of carbon, hydrogen, and oxygen in the compound:** - **Carbon Analysis:** - Mass of \( CO_2 \) produced: 0.5059 g - Since each mole of \( CO_2 \) contains one mole of carbon, find the moles of carbon: \[ \text{Moles of C} = \frac{\text{Mass of } CO_2}{\text{Molar Mass of } CO_2} = \frac{0.5059 \, \text{g}}{44.01 \, \text{g/mol}} = 0.011497 \, \text{mol} \] - **Hydrogen Analysis:** - Mass of \( H_2O \) produced: 0.2071 g - Since each mole of \( H_2O \) contains two moles of hydrogen, find the moles of hydrogen: \[ \text{Moles of H} = 2 \times \frac{\text{Mass of } H_2O}{\text{Molar Mass of } H_2O} = 2 \times \frac{0.2071 \, \text{g}}{18.02 \, \text{g/mol}} = 0.023003 \, \text{mol} \] - **Oxygen Analysis:** - Use the mass of the compound burned and the

Given, An unknown compound having formula CxHyOz. Mass of the compound = 0.2072 g mass of CO2…

An unknown compound has the formula C HyO₂. You burn 0.2072 g of the compound and isolate 0.5059 g of CO2 and 0.2071 g of H₂O. What is the empirical formula of the compound? If the molar mass is 72.1 g/mol, what is the molecular formula? (Enter the elements in the order: C, H, O.) Empirical formula: Molecular formula:

An unknown compound has the formula C HyO₂. You burn 0.2072 g of the compound and isolate 0.5059 g of CO2 and 0.2071 g of H₂O. What is the empirical formula of the compound? If the molar mass is 72.1 g/mol, what is the molecular formula? (Enter the elements in the order: C, H, O.) Empirical formula: Molecular 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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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

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### Determining Empirical and Molecular Formulas of a Compound

An unknown compound has the formula \( C_xH_yO_z \). You burn 0.2072 g of the compound and isolate 0.5059 g of \( CO_2 \) and 0.2071 g of \( H_2O \). What is the empirical formula of the compound? If the molar mass is 72.1 g/mol, what is the molecular formula?

**Problem:**
(Enter the elements in the order: C, H, O.)

| Empirical formula: | [---Text Box for Answer---] |
| Molecular formula: | [---Text Box for Answer---] |

In this problem, the goal is to find both the empirical and molecular formulas of the unknown compound. Let's break down the steps necessary to solve this problem.

#### Step-by-Step Method:

1. **Determine the amount of carbon, hydrogen, and oxygen in the compound:**

- **Carbon Analysis:**
- Mass of \( CO_2 \) produced: 0.5059 g
- Since each mole of \( CO_2 \) contains one mole of carbon, find the moles of carbon:
\[
\text{Moles of C} = \frac{\text{Mass of } CO_2}{\text{Molar Mass of } CO_2} = \frac{0.5059 \, \text{g}}{44.01 \, \text{g/mol}} = 0.011497 \, \text{mol}
\]

- **Hydrogen Analysis:**
- Mass of \( H_2O \) produced: 0.2071 g
- Since each mole of \( H_2O \) contains two moles of hydrogen, find the moles of hydrogen:
\[
\text{Moles of H} = 2 \times \frac{\text{Mass of } H_2O}{\text{Molar Mass of } H_2O} = 2 \times \frac{0.2071 \, \text{g}}{18.02 \, \text{g/mol}} = 0.023003 \, \text{mol}
\]

- **Oxygen Analysis:**
- Use the mass of the compound burned and the

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