None 11.30 Carbon tetrachloride, CCl4, and chloroform, CHCl3, arecommon organic liquids. Carbon tetrachloride's normalboiling point is 77 °C; chloroform's normal boiling pointis 61 °C. Which statement is the best explanation of thesedata? (a) Chloroform can hydrogen-bond, but carbon tet-rachloride cannot. (b) Carbon tetrachloride has a largerdipole moment than chloroform. (c) Carbon tetrachlorideis more polarizable than chloroform.ahedral nolvatomic

The difference in boiling points between carbon tetrachloride (CCl4) and chloroform (CHCl3) can be…

Answered: 11.30 Carbon tetrachloride, CCl4, and…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 93QAP

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Define the normal boiling point of water. Why does a sample of boiling water remain at the same temperature until all the water has been boiled? Define the normal freezing point of water. Sketch a representation of a heating/cooling curve for water, marking clearly the normal freezing and boiling points.
(a) Temperature dependence of the vapor pressure of ethylene log p (mm Hg) = - 834.13 / T + 1.75 log T - 8.375 x 10-3 T + 5.3234 , which gives the temperature dependence of the molar enthalpy of vaporization derive the equation. (b) Calculate the molar enthalpy of evaporation at -103.9 oC, the normal boiling point of ethylene. Note: Use the equation that gives the temperature dependence of ΔHvap= a + bT + cT2+ ….enthalpy.
The vapor pressure of ammonia at –50°C is 0.4034 atm; at 0°C, it is 4.2380 atm. (a) Calculate the molar enthalpy of vaporization (AHvap) of ammonia. (b) Calculate the normal boiling temperature of NH3(€).
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Arrange the following in terms of increasing boiling point using (<) less than equality.
please explain
3. (a) The Lattice enthalpy for the solid ionic compound AgBr is +900. kJ/mole. Write the chemical equation that corresponds to the Lattice Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large positive number. (b) The hydration enthalpy for AgBris -821 kJ/mole. Write the chemical equation that corresponds to the Hydration Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large negative number. (c) Would you expect this compound to be soluble in water? Why/Why not? Calculate anything you need in order to figure this out, and explain your answer.
(3) Vapor pressure of liquid ethanol is 7291 Pa at 20°C. (a) one student reports that the vapor pressure is 31741 Pa at 52°C. Another student reports it to be 31741 Pa at 502°C. Which of the results is correct? Why? (b) calculate the normal boiling temperature of ethanol (assume Patm=101,325Pa).
Calculate the cryoscopic and ebullioscopic constants for liquid bromine, Br2. You will need the following data: 8.89 K/molal (Kf); 4.95 K/molal (Kb)ΔfusH: 10.57 kJ/mol; MP: 27.2°CΔvapH: 29.56 kJ/mol; BP: 58.78°C
What is Δq for the vaporization of 50.0 g of Compound A (76.03 g/mol; ΔHvap is 31.6 kJ/mol)?
ow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take [References] Use the References to access important values if needed for this question. Liquid propanol (C3H¬OH) has a normal boiling point of 97.2 °C and liquid pentanol (C;H|OH) has a normal boiling point of 138 °C. (a) In which of the two are the intermolecular forces the weakest? (b) Which of the two would you expect to have the highest viscosity at 25 °C? | Submit Answer Try Another Version 1 item attempt remaining ot pt Previous Cengage Learning | Cengage Technical Support 888 & %23 24 7 8 3. 4 R T. Y K D C V
You take a sample of water that is at room temperature andin contact with air and put it under a vacuum. Right away,you see bubbles leave the water, but after a little while, thebubbles stop. As you keep applying the vacuum, more bubblesappear. A friend tells you that the first bubbles werewater vapor, and the low pressure had reduced the boilingpoint of water, causing the water to boil. Another friendtells you that the first bubbles were gas molecules from theair (oxygen, nitrogen, and so forth) that were dissolvedin the water. Which friend is mostly likely to be correct?What, then, is responsible for the second batch of bubbles?

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