acetone and ethanol Choose one or more: A. London dispersion B. dipole–dipole C. hydrogen bonding D. ion-induced dipole
1 answer:
Explanation:
The weak intermolecular forces which can arise either between nucleus and electrons or between electron-electron are known as dispersion forces. These forces are also known as London dispersion forces and these are temporary in nature.
Dipole-dipole interactions are defined as the interactions that occur when partial positive charge on an atom is attracted by partial negative charge on another atom.
When a polar molecules produces a dipole on a non-polar molecule through distribution of electrons then it is known as dipole-induced forces.
Hydrogen bonding is defined as a bonding which exists between a hydrogen atom and an electronegative atom like O, N and F.
Chemical formula of acetone is . Due to the presence of oxygen atom there will be partial positive charge on carbon and a partial negative charge on oxygen atom. Hence, dipole-dipole forces will exist in a molecule of acetone.
Whereas hydrogen bonding will exist in a molecule of ethanol (). Since, hydrogen atom is attached with electronegative oxygen atom.
Whereas London dispersion forces will also exist in both acetone and ethanol molecule.
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<h2>Hello!</h2>
The answer is: -97.37° C
<h2>Why?</h2>According to the Charles and Gay-Lussac's Law we have that:
Where:
<em>v</em> is the volume of the gas
<em>t</em> is the temperature of the gas
<em>k </em>is the proportionality constant
From the Gay-Lussac's Law we also have the following relation:
Since we need to find the new temperature (T2) we can use the last equation:
We are asked to find the temperature in Celsius degrees, so, we must convert the result (in K) to Celsius degrees:
So, the temperature is -97.37° C
Have a nice day!