**Freezing Point Depression Experiment**The freezing point of ethanol, \( \text{CH}_3\text{CH}_2\text{OH} \), is \(-117.300 \, ^\circ\text{C}\) at 1 atmosphere. The cryoscopic constant (\( K_f \)) for ethanol is \( 1.99 \, ^\circ\text{C/m} \).In a laboratory experiment, students synthesized a new compound and observed that when \( 13.92 \) grams of the compound were dissolved in \( 224.6 \) grams of ethanol, the solution began to freeze at \(-117.438 \, ^\circ\text{C}\). The compound was also found to be nonvolatile and a non-electrolyte.**Question:**What is the molecular weight they determined for this compound?\[ \_\_\_\_\_ \, \text{g/mol} \] **Boiling Point Elevation/Freezing Point Depression**\[ \Delta T = m \, K \]Where, for freezing point depression:\[ \Delta T = T(\text{pure solvent}) - T(\text{solution}) \]And for boiling point elevation:\[ \Delta T = T(\text{solution}) - T(\text{pure solvent}) \]- \( m = \) (# moles solute / Kg solvent)- \( K_b = \) boiling point elevation constant.- \( K_f = \) freezing point depression constant.\( K_b \) and \( K_f \) depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow.| Solvent | Formula | \( K_b (°C/m) \) | \( K_f (°C/m) \) ||--------------|--------------|-----------------|-----------------|| Water | \( \text{H}_2\text{O} \) | 0.512 | 1.86 || Ethanol | \( \text{CH}_3\text{CH}_2\text{OH} \) | 1.22 | 1.99 || Chloroform | \( \text{CHCl}_3 \) | 3.67 | || Benzene | \( \text{C}_6\text{H}_6 \) | 2.53 | 5.12 || Diethyl ether| \( \text{CH}_3\text{CH}_2\text{OCH}_2\text{CH}_3 \) | 2.02 | |

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The freezing point of ethanol, CH3CH₂OH, is -117.300 °C at 1 atmosphere. Kf(ethanol) = 1.99 °C/m In a laboratory experiment, students synthesized a new compound and found that when 13.92 grams of the compound were dissolved in 224.6 grams of ethanol, the solution began to freeze at -117.438 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol

The freezing point of ethanol, CH3CH₂OH, is -117.300 °C at 1 atmosphere. Kf(ethanol) = 1.99 °C/m In a laboratory experiment, students synthesized a new compound and found that when 13.92 grams of the compound were dissolved in 224.6 grams of ethanol, the solution began to freeze at -117.438 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol

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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