The boiling point is always higher than the melting point.
Yes, because the melting point depends on the strength of the intermolecular forces, which are different for different molecules and compounds. Stronger intermolecular forces mean a higher melting point.
The magnesium chloride solution has a higher boiling point.
The molecular mass of iodobutane is higher so density and boiloing point also higher than chlorobutane.
The CH3CH2CH2CH2OH molecules can form strong hydrogen bonds with each other due to the presence of the lone pairs of electrons on O and the H atom which is bonded to the O atom, while CH3CH2CH2CH2SH molecules are unable to due to the absence of H atoms bonded to either F, O or N atoms. As such, more heat energy is required to overcome the stronger hydrogen bonds and thus CH3CH2CH2CH2OH has a higher bioling point.
due to intermolecular hydrogen bonding
Boiling point you mean, and H20 has a higher BP
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no..ethers are always low in boiling point than alcohol due to alcohols hydrogen bonds
Due to the absence of replaceable hydrogen atoms
The boiling point of water will be greatest at that point on Earth that is the closest to sea level. Boiling point of water depends on the atmospheric pressure. The boiling point of water varies depending on the weather. At low atmospheric temperatures due to weather or due to being up a mountain, the water will boil below its "normal" boiling point of 100 oC
The point elasticity of supply is a measure of the rate of response of quantity demand due to a price change. The higher the elasticity, the more sensitive the sellers are to these changes.
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Since oxygen has a higher electronegativity than nitrogen, the hydroxyl radical is more polar than the amide radical, and hence, creates a stronger electrostatic attraction between molecules and consequently a higher boiling point.
You mean rise not rinse. Higher in a narrow tube due to capillary action.
Yes, due to higher no of solute particles the total kinetic energy will be higher, its proof is that such solutions freeze at lower temperature than a dilute solution (depression of freezing point).
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