At room temperature, the vapor pressure pattern of the following compounds isC,H16СНОНH3C`CH3acetoneethanolheptane100 g/mol58 g/mol46 g/molWhich one of the following statements is FALSE:а.a substance with lower vapor pressure is held together by stronger binding forces.b.ethanol has the lowest vapor pressure, and London force explains why.с.ethanol has the lowest vapor pressure, and hydrogen bonding explains why, even though it has the weakest Londonforce.d. The reason that heptane has a lower vapor pressure than acetone is because heptane is heavier and has substantiallygreater London dispersion force, even though acetone has dipole-dipole interactions in its favor.

A substance with strong bonding forces will not vaporize quickly and hence will have a lower vapor…

At room temperature, the vapor pressure pattern of the following compounds is > C,H16 > C,H;OH H3C° `CH3 acetone ethanol heptane 100 g/mol 58 g/mol 46 g/mol Which one of the following statements is FALSE: a substance with lower vapor pressure is held together by stronger binding forces. b. ethanol has the lowest vapor pressure, and London force explains why. ethanol has the lowest vapor pressure, and hydrogen bonding explains why, even though it has the weakest London force. а. с. d. The reason that heptane has a lower vapor pressure than acetone is because heptane is heavier and has substantially greater London dispersion force, even though acetone has dipole-dipole interactions in its favor.

At room temperature, the vapor pressure pattern of the following compounds is > C,H16 > C,H;OH H3C° `CH3 acetone ethanol heptane 100 g/mol 58 g/mol 46 g/mol Which one of the following statements is FALSE: a substance with lower vapor pressure is held together by stronger binding forces. b. ethanol has the lowest vapor pressure, and London force explains why. ethanol has the lowest vapor pressure, and hydrogen bonding explains why, even though it has the weakest London force. а. с. d. The reason that heptane has a lower vapor pressure than acetone is because heptane is heavier and has substantially greater London dispersion force, even though acetone has dipole-dipole interactions in its favor.

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

NOTE: please base the value of boiling and freezing point, and Kb on the given table.
O Macmillan Learning The vapor pressure of ethanol, CH₂CH₂OH, at 40.0 °C is 17.88 kPa. If 2.25 g of ethanol is enclosed in a 3.00 L container, how much liquid will be present? mass of liquid: g
How to identify which one is the highest boiling point?
10- Which of the following should have the lowest boiling point? a) O HCI b) O H20 C) O PH3 d) O H2S e) SİH4 Boş bırak KÖnceki 10/20 Sonraki> Ka
Select the appropriate options to identify which compound in the following pair has the lower freezing point and identify the strongest intermolecular forces for that compound: CH3CH₂CH₂OH (n-propanol) or CH3CH₂CH3 (propane) has the lower freezing point. The strongest intermolecular forces of the compound with the lower freezing point are 1. CH3CH₂CH₂OH (n-propanol) 2. CH3CH₂CH3 (propane) 3. ion-dipole forces 4. hydrogen-bonding forces 5. dipole-dipole forces 6. ion-induced dipole forces 7. dipole-induced dipole forces 8. dispersion forces
Use the following vapor pressure data to answer the questions: A B Liquid C7H16 C₂H5Br Vapor Pressure, torr Temperature, °C 400 78.0 400 21.0 (1) In which liquid are the intermolecular attractive forces the weakest ? (2) The vapor pressure of C7H16 at 21.0 °C would be than 400 torr.
I'm lost on where to start with this question
please,don't provied handwriting solution.
What is the answer for question 15?
Using the graphic below, what can be said about the strength of the intermolecular forces (IMFS) of water in the Step 2 compared to Step 4? Heating Curve of Water 100 50 Time ---> O The IMFS solid water are stronger in liquid water and this is seem by the shorter length of Step 2 compared to Step 4 O The IMFS of liquid water are stronger than in solid water and this is seen by the longer length of the segment of Step 4 compared to Step 2 The IMFS of solid water are stronger than in liquid water and this is seen by the longer length of the segment of Step 4 compared to Step 2 The IMFS of liquid water are stronger in solid water and this is seem by the shorter length of Step 2 compared to Step 4 (0.) amaradL
24 Feb 2021 2odium chloride (NaCI) is completely saluble in water. What is responsible for its solubility in water? A. Na+ and Clions are favorable sites for H-bonding to torm. В. The presence of charged ends in NaCl enables dipole-dipole interaction with water. e lons in Načl participate in on-induced dipole attractions with water. C. D. London dispersion forces in NaCl predominate leading to strong dipole interactions with water. 5. Kenon (Xe) has a greater atomic weight than Neon (Ne). Xe has 131.3 amu while Ne has 20.2 amu, The melting points are 166.1K and 27.3K, respectively. How do intermolecular forces account for the difference? A. Dipole- dipole interaction is greater in Xe than Ne so more energy is needed to break the bonds. B. H-bonding is greater for substances with higher atomic weight so greater energy is needed to change Xe to vapor. C. Atomic weight increases the chance of lesser dispersion forces so greater energy is needed to separate Xe atoms to change to vapor. D.…
The vapor of liquid bismuth is 400 mm Hg at 1.72x10^3 K. Assuming that it’s molar heat of vaporization is constant at 184 kj/mol, the vapor pressure of liquid Bi is ____ mm Hg at a temperature of 1.70x10^3. The normal boiling point of liquid ethane thiol is 308 K. Assuming that its molar heat of vaporization is constant at 26.7 kj/mol, the boiling pint of C2H5SH when the external pressure is 0.753 atm is ____ K.