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The boiling point of ethanol CH3CH,OH is 78.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is saccharin How many grams of saccharin, C-H&NOS (183.2 g/mol), must be dissolved in 220.0 grams of ethanol to raise the boiling point by 0.500 °C ? Refer to the table for the necessary boiling on freezing point constant. Solvent Formula K CC/m) Kf°C/m) Water H20 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCI3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH;CH2OCH2CH3 2.02 g saccharin Submit Answer Retry Entire Group 9 more group attempts remaining

The boiling point of ethanol CH3CH,OH is 78.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is saccharin How many grams of saccharin, C-H&NOS (183.2 g/mol), must be dissolved in 220.0 grams of ethanol to raise the boiling point by 0.500 °C ? Refer to the table for the necessary boiling on freezing point constant. Solvent Formula K CC/m) Kf°C/m) Water H20 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCI3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH;CH2OCH2CH3 2.02 g saccharin Submit Answer Retry Entire Group 9 more group attempts remaining

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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### Boiling Point Elevation and Freezing Point Depression The boiling point of ethanol (CH₃CH₂OH) is 78.50°C at 1 atmosphere. Saccharin is a nonvolatile, nonelectrolyte that dissolves in ethanol. **Problem Statement:** How many grams of saccharin (C₇H₅NO₃S, 183.2 g/mol) must be dissolved in 220.0 grams of ethanol to raise the boiling point by 0.500°C? Use the table below for the necessary boiling or freezing point constant. #### Table of Solvent Properties | Solvent | Formula | \( K_b \) (°C/m) | \( K_f \) (°C/m) | |---------------|-----------------|------------------|------------------| | Water | H₂O | 0.512 | 1.86 | | Ethanol | CH₃CH₂OH | 1.22 | 1.99 | | Chloroform | CHCl₃ | 3.67 | | | Benzene | C₆H₆ | 2.53 | 5.12 | | Diethyl ether | CH₃CH₂OCH₂CH₃ | 2.02 | | **Input Box:** \[ \text{g saccharin} \] **Buttons:** - Submit Answer - Retry Entire Group (9 more attempts remaining) **Additional Information:** - This exercise is about calculating the amount of solute needed to achieve a desired change in the boiling point of a solvent, using colligative properties. - The table provides crucial constants needed for calculating colligative properties: the boiling point elevation constant (\( K_b \)) and freezing point depression constant (\( K_f \)) for various solvents. - The task emphasizes the understanding of how solute properties such as mass and molar mass affect the boiling point when a solute is added to a solvent. This problem helps to reinforce the application of colligative properties in practical scenarios.
Transcribed Image Text:### Boiling Point Elevation and Freezing Point Depression The boiling point of ethanol (CH₃CH₂OH) is 78.50°C at 1 atmosphere. Saccharin is a nonvolatile, nonelectrolyte that dissolves in ethanol. **Problem Statement:** How many grams of saccharin (C₇H₅NO₃S, 183.2 g/mol) must be dissolved in 220.0 grams of ethanol to raise the boiling point by 0.500°C? Use the table below for the necessary boiling or freezing point constant. #### Table of Solvent Properties | Solvent | Formula | \( K_b \) (°C/m) | \( K_f \) (°C/m) | |---------------|-----------------|------------------|------------------| | Water | H₂O | 0.512 | 1.86 | | Ethanol | CH₃CH₂OH | 1.22 | 1.99 | | Chloroform | CHCl₃ | 3.67 | | | Benzene | C₆H₆ | 2.53 | 5.12 | | Diethyl ether | CH₃CH₂OCH₂CH₃ | 2.02 | | **Input Box:** \[ \text{g saccharin} \] **Buttons:** - Submit Answer - Retry Entire Group (9 more attempts remaining) **Additional Information:** - This exercise is about calculating the amount of solute needed to achieve a desired change in the boiling point of a solvent, using colligative properties. - The table provides crucial constants needed for calculating colligative properties: the boiling point elevation constant (\( K_b \)) and freezing point depression constant (\( K_f \)) for various solvents. - The task emphasizes the understanding of how solute properties such as mass and molar mass affect the boiling point when a solute is added to a solvent. This problem helps to reinforce the application of colligative properties in practical scenarios.
**Laboratory Experiment: Determining the Molecular Weight of a Compound Using Diethyl Ether as Solvent** The common laboratory solvent **diethyl ether** (often referred to simply as "ether") is frequently used to purify substances dissolved in it. The vapor pressure of diethyl ether, with the chemical formula \( \text{C}_2\text{H}_5\text{OC}_2\text{H}_5 \), is 463.57 mm Hg at 25 °C. In this laboratory experiment, students synthesized a new compound. They discovered that when 26.16 grams of this compound were dissolved in 274.2 grams of diethyl ether, the vapor pressure of the solution was measured to be 451.84 mm Hg. The compound was also confirmed to be nonvolatile and a non-electrolyte. **Objective:** Determine the molecular weight (MW) of the synthesized compound. **Given:** - Diethyl ether: \( \text{C}_2\text{H}_5\text{OC}_2\text{H}_5 \), Molecular Weight = 74.12 g/mol **Calculation Required:** - Calculate the molecular weight (MW) of the compound using the data provided. Input your calculated molecular weight in the box provided and click "Submit Answer" to check the result. You have 9 more group attempts remaining. **Note:** Ensure you utilize all necessary references to access important values if needed for this question. --- **Instructions for input:** MW = _______ g/mol You can retake or retry the group activity if required by clicking "Retry Entire Group." **Navigation:** Use the "Previous" and "Next" buttons to move between questions. Click "Save and Exit" if you need to leave and return later. **Technical Support:** For assistance, contact Cengage Learning | Cengage Technical Support.
Transcribed Image Text:**Laboratory Experiment: Determining the Molecular Weight of a Compound Using Diethyl Ether as Solvent** The common laboratory solvent **diethyl ether** (often referred to simply as "ether") is frequently used to purify substances dissolved in it. The vapor pressure of diethyl ether, with the chemical formula \( \text{C}_2\text{H}_5\text{OC}_2\text{H}_5 \), is 463.57 mm Hg at 25 °C. In this laboratory experiment, students synthesized a new compound. They discovered that when 26.16 grams of this compound were dissolved in 274.2 grams of diethyl ether, the vapor pressure of the solution was measured to be 451.84 mm Hg. The compound was also confirmed to be nonvolatile and a non-electrolyte. **Objective:** Determine the molecular weight (MW) of the synthesized compound. **Given:** - Diethyl ether: \( \text{C}_2\text{H}_5\text{OC}_2\text{H}_5 \), Molecular Weight = 74.12 g/mol **Calculation Required:** - Calculate the molecular weight (MW) of the compound using the data provided. Input your calculated molecular weight in the box provided and click "Submit Answer" to check the result. You have 9 more group attempts remaining. **Note:** Ensure you utilize all necessary references to access important values if needed for this question. --- **Instructions for input:** MW = _______ g/mol You can retake or retry the group activity if required by clicking "Retry Entire Group." **Navigation:** Use the "Previous" and "Next" buttons to move between questions. Click "Save and Exit" if you need to leave and return later. **Technical Support:** For assistance, contact Cengage Learning | Cengage Technical Support.
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