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11.21 Butane and 2-methylpropane, whose space-filling models are shown, are both nonpolar and have the same molecular formula, yet butane has the higher boiling point (-0.5 °C compared to -11.7 °C).

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Sep 19, 2013 · D) always equal to the vapor pressure of the liquid at a given temperature. E) independent of the pressure exerted on the liquid. ANS: C PTS: 1 DIF: easy REF: 11.2 OBJ: Define boiling point. TOP: phases | phase transitions 13. Which one of the following liquids would you expect to have the highest vapor pressure at room temperature?

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Lowest to highest I got this wrong twice. I put CH3OH Low CH3CL Med CH4 High wrong CH3Cl low 11.56 F boiling point CH3OH med 149 F boiling point CH4 257.8 F boiling point all these were wrong. Please explain what I am doing wrong. THANKS:)

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____ 20. Which substance would be expected to have the highest heat of vaporization? a. F 2 b. CCl 4 c. C 2 H 6 d. CH 3 OCH 3 e. CH 2 OHCH 2 OH ____ 21. Some solids can be converted directly to the vapor phase by heating. The process is called _____. a. fusion b. sublimation c. vaporization d. condensation e. distillation ____ 22.

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Aug 31, 2015 · Main Difference – Boiling Point vs. Melting Point. Melting point and boiling point both describe temperatures at which phase changes occur in substances.The main difference between boiling point and melting point is that the melting point is defined as the temperature at which solid and liquid phases are in equilibrium, whereas the boiling point is the temperature at which the vapour ...

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In general, ionic compounds will have higher boiling points than those of dipole-dipole interaction compounds. So, the compound above that will have the highest melting point will certainly be an ionic compound, either $\ce{NaCl}$, $\ce{CaF2}$ or $\ce{SrCl2}$.

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Liquids that contain dissolved substances have increased boiling points. This effect is called boiling point elevation, and it's an example of a colligative property -- a property that depends on the number of solute and solvent molecules but not the identity of the solute.

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Consequently, we expect intermolecular interactions for n-butane to be stronger due to its larger surface area, resulting in a higher boiling point. The overall order is thus as follows, with actual boiling points in parentheses: propane (−42.1°C) < 2-methylpropane (−11.7°C) < n -butane (−0.5°C) < n -pentane (36.1°C).

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Feb 22, 2017 · A substance with a lower boiling point has higher volatility and vapour pressure. The volatility of a substance is affected by the strength of intermolecular forces . For example, water is not readily volatile at room temperature and needs to be heated in order to evaporate.

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This is why they have so much higher melting points and boiling points. Substance: formula: Type of bonding, structure and attractive forces operating: Melting point K (Kelvin) = o C + 273: Energy needed to melt substance: Boiling point K (Kelvin) = o C + 273: Energy needed to boil substance: methane: CH 4

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Consider the boiling points of increasingly larger hydrocarbons. More carbons means a greater surface area possible for hydrophobic interaction, and thus higher boiling points. As you would expect, the strength of intermolecular hydrogen bonding and dipole-dipole interactions is reflected in higher boiling points.
May 28, 2008 · The boiling point of water (H2O) is higher than the boiling point of hydrogen sulfide (H2S)Is it because the water molecule is less polar, more covalent, ionic, or more polar? Answer Save 6 Answers
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Sep 26, 2012 · The highest boiling point is for CH3Cl among the given compounds. See, there are four types of IMF, 1. London force. 2. Dipole - Dipole. 3. Dipole induced Dipole and. 4. H bonding. Electrostatic forces don't come under IMF as they are b/w opp. charged ions. Amongst the four, the strongest is H bonding, which is a special case of Dipole - Dipole.

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In an ideal situation, the temperature in the distillation flask would be equal to the boiling point of the mixture of liquids and the temperature at the top of the fractionating column would be equal to the boiling point of the lower boiling compound; all of the lower boiling compound would be distilled away before any of the higher boiling ...
= C = O = H: methyl ether (C 2 H 6 O) The normal boiling point of methyl ether is -25 o C (i.e., a gas at room temperature). The relatively weak dipole-dipole forces and London dispersion forces between molecules results in a much lower normal boiling point compared to ethyl alcohol.