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 Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.87QE

See similar textbooks

Similar questions

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.
(c). 12.39 Which member in each pair of liquids has the lower vapor pressure at a given temperature? Explain. (a) HOCH,CH,OH or CH,CH,CH,OH (b) CH,COOH or (CH,),C=0 (c) HF or HCI
The phase diagram for helium is shown. Liquid helium can exist in two possible forms; Helium II and Helium I. Explain. (i) What is the maximum temperature at which Helium – II can exist? (ii)What is the minimum pressure at which solid helium can exist? (iii) What is the normal boiling point for Helium – 1? (iv) Can solid helium sublime?
(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.
12.39 Which member in each pair of liquids has the lower vapor pressure at a given temperature? Explain. (a) HOCH,CH,OH or CH,CH,CH,OH (b) CH;COOH or (CH;),C=0 1. (c) HF or HCI
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(€).
2.) Determine the freezing point of benzene (78.11 g/mol) at 100 atm if the normal freezing point is 5.5°C, the enthalpy of fusion for benzene is 9.937 kJ/mol. Assume that the enthalpy is independent of the temperature. The densities of solid and liquid benzene are 1.012 g/cm3 and 0.879 g/cm3. A. 282°C B. 8.2°C C. 278.68°C D.) 5.5 °C E. 5.6°C
In benzene, dimerization occurs with benzene due to hydrogen bonding. In 110 g of benzene, 1.70g of acetic acid is dissolved that increases the boiling point by 0.40 oC. What is the expected degree of association of acetic acid? (Use Kb=2.57 Kg mol-1 )?
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 AgBr is -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.…
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
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.
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?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS