Consider the difference between boiling water and boiling oil. Water boils at 100°C, while oil requires a much highertemperature. This difference is due to the intermolecular forces between the molecules. Water molecules are heldtogether by hydrogen bonds, which are stronger than the Van der Waals forces in oil. As a result, more energy is neededto break the bonds in water, leading to its lower boiling point. Which statement best explains the effect of intermolecularforces on boiling points?A) Stronger intermolecular forces result in higher boiling points.B) All liquids boil at the same temperature regardless of intermolecular forces.C) Weaker intermolecular forces result in higher boiling points.D) Intermolecular forces have no effect on boiling points.

There are four types of intermolecular forces.Ionic forces: This is the interaction between charged…

Answered: Consider the difference between boiling…

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...

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The vapor pressure of acetone (C3H6O) are 400 torr at 39.5 oC and 760 torr at 56.5oC. Determine the boiling point of acetone and its enthalpy of vaporization (Hvap) in kJ/mol. (R = 8.314 J/mol.K)
Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.05 kg of water decreased from 117 °C to 56.5 °C. Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C
Which of these statements about hydrogen bonds is not true? Individual hydrogen bonds in liquid water exist for less than a second. Hydrogen bonds do not account for the anomalously high boiling point of water. O In liquid water, the average water molecule forms hydrogen bonds with three to four other water molecules. Individual hydrogen bonds are much weaker than covalent bonds. The strength of a hydrogen bond depends on the linearity of the three atoms involved in the bond.
- Suppose a small sample of pure X is held at -236.°C and 2.0 atm. What will be the state of the sample (solid, liquid, or gas)? - Suppose the temperature is held constant at -236.°C but the pressure is decreased by 1.2 atm. What will happen to the sample (nothing, it will melt, it will freeze, it will boil, it will condense, it will sublime, or it will deposit)? - Suppose, on the other hand, the pressure is held constant at 2.0 atm but the temperature is increased by 137°C. What will happen to the sample (nothing, it will melt, it will freeze, it will boil, it will condense, it will sublime, or it will deposit)? All these are part of one question.
Liquid butane is used in cigarette lighters. The boiling point of butane at 1 atm pressure is -1.0 °C and its ∆H(vap) is 22.44 kJ/mol. R = 8.314 ×10⁻³ kJ/mol･K. Calculate the pressure (in atm) of the butane in the lighter at 19.5 °C.
Determine the chemical formulas for the two compounds. ОН A A: В: Based on their structures, which compound will have the higher boiling point?
The vapor pressure of liquid carbon disulfide, CS2, is 100. mm Hg at 268 K. A 0.261 g sample of liquid CS2 is placed in a closed, evacuated 400. mL container at a temperature of 268 K. Assuming that the temperature remains constant, will all of the liquid evaporate? What will the pressure in the container be when equilibrium is reached? mm Hg
Which should have a higher enthalpy of vaporization, CF4 or CBr4? Explain the role of intermolecular forces in your decision.
Copper, Cu, crystallizes in a face centered cubic unit cell. The density of the metal is 8.96 g/cm 3. A scientist believes that the radius of one Cu atom is 1.321 x 10 - 8 cm. What is the length of cell, calculate the volume of the unit cell by cubing it, calculate the mass of a unit cell, and What is the mass of each atom? He uses this number to calculate Avogadro's number. What number does he get? (Hint: It is not 6.02 x 10 23.).
The strongest intermolecular interactions between pentane (C 5H 12) molecules arise from: O dispersion forces. covalent bond forces. dipole-dipole attraction. hydrogen bonding. ionic interactions. Previous
Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.45 kg of water decreased from 109 °C to 40.5 °C. Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C kJ

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