Identify the strongest attractive forces between the particles of each of the following A.CH3OH B.CO C.CF4 D.CH3-CH3
2 answers:
Answer: A) hydrogen bonding, B) dipole-dipole forces, C) London dispersion forces and D) London dispersion forces.
Explanation: Methanol is a polar covalent molecule means it has dipole-dipole forces of attraction. Since, hydrogen is bonded to more electron negative oxygen atom, this molecule has hydrogen bonding. So, strongest attractive forces for this molecule are hydrogen bonding.
CO is a polar covalent molecule and so it has dipole-dipole forces of attraction.
has four polar covalent bonds but the over all molecule is nonpolar as the dipole moment of one C-F bond is canceled by its opposite C-F bond as the molecule is tetrahedral. Being nonpolar, the molecule has london dispersion forces only.
Ethane is also a nonpolar molecule and so it has london dispersion forces.
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Considering the definition of STP conditions, 3.35 moles of helium are contained within the balloon.
<h3>Definition of STP condition</h3>The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C are used and are reference values for gases. And in these conditions 1 mole of any gas occupies an approximate volume of 22.4 liters.
<h3>Amount of moles of helium within the balloon</h3>In this case, you know that scientist fills a large, tightly sealed balloon with 75,000 mL of helium at STP.
So, you can apply the following rule of three: if by definition of STP conditions 22.4 liters are occupied by 1 mole of helium, 75 L (75 L= 75000 mL, being 1 L= 1000 L) are occupied by how many moles of helium?
<u><em>amount of moles of helium= 3.35 moles</em></u>
Finally, 3.35 moles of helium are contained within the balloon.
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