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What is the boiling point of a solution composed of 21.0 g of urea, (NH₂)2CO, in 0.800 kg of water? (Kbp for H₂O is +0.5121 C/m.) Boiling point = °C Submit Answer Try Another Version 2 item attempts remaining

What is the boiling point of a solution composed of 21.0 g of urea, (NH₂)2CO, in 0.800 kg of water? (Kbp for H₂O is +0.5121 C/m.) Boiling point = °C Submit Answer Try Another Version 2 item 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
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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 Problem **Problem Statement:** What is the boiling point of a solution composed of 21.0 g of urea, \( (NH_2)_2CO \), in 0.800 kg of water? - \( K_{bp} \) for \( H_2O \) is \( +0.5121 \,^\circ C/m \). **Input Fields:** - **Boiling Point:** [  ] **Interface Options:** - **Submit Answer** button - **Try Another Version** button **Attempts Remaining:** - 2 item attempts remaining ### Explanation: This exercise involves calculating the boiling point elevation of a solution using the formula: \[ \Delta T_b = i \cdot K_{bp} \cdot m \] Where: - \( \Delta T_b \) is the boiling point elevation. - \( i \) is the van 't Hoff factor (1 for urea since it does not ionize). - \( K_{bp} \) is the ebullioscopic constant (\( 0.5121 \,^\circ C/m \) for water). - \( m \) is the molality of the solution, calculated by dividing moles of solute by kilograms of solvent. To solve this problem: 1. Calculate the moles of urea from its given mass. 2. Determine the molality of the solution. 3. Use the boiling point elevation formula to calculate the new boiling point of water.
Transcribed Image Text:### Boiling Point Elevation Problem **Problem Statement:** What is the boiling point of a solution composed of 21.0 g of urea, \( (NH_2)_2CO \), in 0.800 kg of water? - \( K_{bp} \) for \( H_2O \) is \( +0.5121 \,^\circ C/m \). **Input Fields:** - **Boiling Point:** [  ] **Interface Options:** - **Submit Answer** button - **Try Another Version** button **Attempts Remaining:** - 2 item attempts remaining ### Explanation: This exercise involves calculating the boiling point elevation of a solution using the formula: \[ \Delta T_b = i \cdot K_{bp} \cdot m \] Where: - \( \Delta T_b \) is the boiling point elevation. - \( i \) is the van 't Hoff factor (1 for urea since it does not ionize). - \( K_{bp} \) is the ebullioscopic constant (\( 0.5121 \,^\circ C/m \) for water). - \( m \) is the molality of the solution, calculated by dividing moles of solute by kilograms of solvent. To solve this problem: 1. Calculate the moles of urea from its given mass. 2. Determine the molality of the solution. 3. Use the boiling point elevation formula to calculate the new boiling point of water.
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