Question:
Calculate the molal depression constant of a solvent which has freezing point \(16.6^{\circ}\mathrm{C}\) and latent heat of fusion \(180.75\mathrm{J / g}\).
Calculate the molal depression constant of a solvent which has freezing point \(16.6^{\circ}\mathrm{C}\) and latent heat of fusion \(180.75\mathrm{J / g}\).
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\(K_f\) has units K·kg/mol. Freezing point must be in Kelvin.
Updated On: Apr 20, 2026
- 2.68
- 3.86
- 4.68
- 2.86
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The Correct Option is B
Solution and Explanation
Step 1: Understanding the Concept:
Molal depression constant \(K_f = \frac{RT_f^2}{1000 \times L_f}\).
Step 2: Detailed Explanation:
\(T_f = 16.6 + 273 = 289.6\) K.
\(L_f = 180.75\) J/g.
\(R = 8.314\) J/K·mol.
\(K_f = \frac{8.314 \times (289.6)^2}{1000 \times 180.75} = \frac{8.314 \times 83868.16}{180750} = \frac{697,000}{180,750} \approx 3.86\).
Step 3: Final Answer:
3.86
Molal depression constant \(K_f = \frac{RT_f^2}{1000 \times L_f}\).
Step 2: Detailed Explanation:
\(T_f = 16.6 + 273 = 289.6\) K.
\(L_f = 180.75\) J/g.
\(R = 8.314\) J/K·mol.
\(K_f = \frac{8.314 \times (289.6)^2}{1000 \times 180.75} = \frac{8.314 \times 83868.16}{180750} = \frac{697,000}{180,750} \approx 3.86\).
Step 3: Final Answer:
3.86
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