4. When performing a melting point on solid compound using a melting point apparatus, two melting point determinations were made. One sample, which was 1 mm in height in the capillary, possessed a melting point of 133.0-133.5°C. The other sample was 10 mm in height. What would you expect the approximate melting point to be for this sample, assuming identical heating rates of 1°/min? (Hint: heat is applied from the bottom of the sample) (Give an actual numerical approximation!)(Hint: at what temperature would 1g of ice start melting at? At what temperature would 10g of ice start melting at?)

4. When performing a melting point on solid compound using a melting point apparatus, two melting point determinations were made. One sample, which was 1 mm in height in the capillary, possessed a melting point of 133.0-133.5°C. The other sample was 10 mm in height. What would you expect the approximate melting point to be for this sample, assuming identical heating rates of 1°/min? (Hint: heat is applied from the bottom of the sample) (Give an actual numerical approximation!)(Hint: at what temperature would 1g of ice start melting at? At what temperature would 10g of ice start melting at?)

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter7: Equilibria In Multiple-component Systems

Section: Chapter Questions

Problem 7.34E

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An unknown compound gave a melting point of 230°C. When the molten liquid solidified, the melting point was redetermined and found to be 131°C. Give a possible explanation for this discrepancy.
11. Melting point temperatures are frequently used to help identify unknown solids and determine their purity. How would the melting point of a pure solid sample compare to that of the same solid contaminated by a solid impurity? Explain.
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wwnorton.com/108921 85% 10/11/21 SCORE ppun21@ole.augie.edu Highest Melting Point CaCl2 NH,OH PCI3 KI Cl2 CH4 SUBMIT ANSWER 4 VIEW SOLUTION 1 3 OF 20 QUESTIONS COMPLETED 56°F Cloudy ^ 10 earch DELL 1. 2.
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Which of the following would be expected to have the highest boiling temperature based on the intermolecular force present for the molecule? CH;OH BH3 OCl, CHA CIF O Type here to search prt se delete home 144 10 esc %24 4. & 7. (@ #3 %23 Tum 5. 8 3D backspace lock 1 Q W R T Y hor enter F G J K ck pause * shift C M alt ctri alt fn
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This yiaph shows how the vapor pressure of three liquids varies with temperature: 900 800. 700. 600 500. 400. 300. - isobutyl alcohol - ethylbenzene - pyridine 200. 100. 100 110 130 140 temperature, °C Use the graph to answer the following questions: most volatile: choose one Which liquid is the most volatile? Which is the least volatile? least volatile: choose one isobutyl alcohol: |°C What is the normal boiling point of each liquid? Note: your answer must be within 1°C of the exact answer to be graded correct. ethylbenzene: °C pyridine: Suppose a beaker of ethylbenzene is put inside a sealed tank containing ethylbenzene gas at 115. degree C and 557. torr. After ten minutes, will there be more liquid in the beaker, less liquid, or the same O more O less O the same amount? vapor pressure, torr
Chemistry 5. You melt the substance and de-coloration occurs. Unfortunately, you weren’t paying attention and miss the melting point. Should you start over or re-melt it? Or both are options ‘okay’? 6. When measuring the melting point of a substance, it suddenly disappears. What has happened? Can you still measure the melting point? If so, how? 7. We should not re-use a sample in a capillary tube for melting point measurement. Why not? 8. It takes significant amount of time for the melting point apparatus to cool down before next measurement if your new sample has a lower melting point than your previous one. What can you do to reduce this time in between measurements when many samples of different melting points are used?
3. Pure benzophenone melts at 48.1°C. Your sample of benzophenone began to freeze at 47.0°C. When you repeated this measurement, the sample again began to freeze at 47.0°C. Give at least two reasonable explanations for this observation.

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