2.00 g of an unknown compound is mixed to form a homogeneous solution with 75.00 g of benzene. This reduces the freezing point from 5.53 to 4.90 °C. What is the molar mass of the compound? AT;= – Kfx m; Kj= 5.12 for benzene

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...
icon
Related questions
Question
**Freezing Point Depression and Molar Mass Calculation**

When 2.00 grams of an unknown compound is mixed with 75.00 grams of benzene, the freezing point of the solution drops from 5.53°C to 4.90°C. To determine the molar mass of the compound, we can use the equation for freezing point depression:

\[
\Delta T_f = -K_f \times m
\]

Where:
- \(\Delta T_f\) is the change in freezing point.
- \(K_f\) is the freezing point depression constant for benzene, given as 5.12°C kg/mol. 
- \(m\) is the molality of the solution.

**Steps to Calculate the Molar Mass:**

1. **Calculate \(\Delta T_f\):**
   \[
   \Delta T_f = 5.53°C - 4.90°C = 0.63°C
   \]

2. **Determine the molality (\(m\)):**
   Use the formula:
   \[
   m = \frac{\Delta T_f}{K_f} = \frac{0.63°C}{5.12°C \, \text{kg/mol}}
   \]

3. **Calculate moles of solute:**
   The molality (\(m\)) is moles of solute per kg of solvent. Use the mass of benzene (75.00 g = 0.075 kg) to find the moles of solute.

4. **Determine the molar mass of the compound:**
   Use the formula:
   \[
   \text{Molar mass} = \frac{\text{mass of solute (in grams)}}{\text{moles of solute}}
   \]

This process will yield the molar mass of the unknown compound.
Transcribed Image Text:**Freezing Point Depression and Molar Mass Calculation** When 2.00 grams of an unknown compound is mixed with 75.00 grams of benzene, the freezing point of the solution drops from 5.53°C to 4.90°C. To determine the molar mass of the compound, we can use the equation for freezing point depression: \[ \Delta T_f = -K_f \times m \] Where: - \(\Delta T_f\) is the change in freezing point. - \(K_f\) is the freezing point depression constant for benzene, given as 5.12°C kg/mol. - \(m\) is the molality of the solution. **Steps to Calculate the Molar Mass:** 1. **Calculate \(\Delta T_f\):** \[ \Delta T_f = 5.53°C - 4.90°C = 0.63°C \] 2. **Determine the molality (\(m\)):** Use the formula: \[ m = \frac{\Delta T_f}{K_f} = \frac{0.63°C}{5.12°C \, \text{kg/mol}} \] 3. **Calculate moles of solute:** The molality (\(m\)) is moles of solute per kg of solvent. Use the mass of benzene (75.00 g = 0.075 kg) to find the moles of solute. 4. **Determine the molar mass of the compound:** Use the formula: \[ \text{Molar mass} = \frac{\text{mass of solute (in grams)}}{\text{moles of solute}} \] This process will yield the molar mass of the unknown compound.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

Blurred answer
Knowledge Booster
Solutions
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY