Answer:
HF
Explanation:
This concept can be understood from the knowledge of Intermolecular forces of attraction.
Intermolecular bonds are Van der Waals forces which are weak forces of attraction joining non-polar and polar molecules together. They exist in the form of London Dispersion Forces and Dipole-dipole attraction.
An example of Dipole-dipole attraction is the hydrogen bond which is a unique dipole-dipole attraction between polar molecules in which a hydrogen atom is directly joined to a highly electronegative atom such as fluorine, oxygen, or nitrogen).
Molecules that possess the characteristics of hydrogen bonding have a higher boiling point. In the given question, only HF undergo hydrogen bond due to the electronegative effect of the fluorine element.
F2 occurs as a weak London dispersion force and it occurs between non-polar molecules.
its is making no net release of carbon dioxide to the atmosphere,especially through offsetting emissions by planting trees
Answer:
4.5 moles of H2O.
Explanation:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
C2H5OH + 3O2 —> 2CO2 + 3H2O
From the balanced equation above,
1 moles of C2H5OH reacted to produce 3 moles of H2O.
Finally, we shall determine the number of mole of H2O produced by the reaction of 1.5 moles of C2H5OH. This can be obtained as follow:
From the balanced equation above,
1 moles of C2H5OH reacted to produce 3 moles of H2O.
Therefore, 1.5 moles of C2H5OH will react to produce = 1.5 × 3/ 1 = 4.5 moles of H2O.
Thus, 4.5 moles of H2O will be produced.
Water, H₂O, will have the highest melting point.
Explanation:
So here we have listed the hydrides of oxygen, sulphur, selenium and tellurium.
From this elements oxygen have the highest electronegativity and as a consequence the oxigen hydride (water, hydrogen dioxide) it is able to form hydrogen bonds between molecules. So you need more energy to overcome the interactions between molecules in water that for the other compounds.
Water, H₂O, will have the highest melting point between the listed hydrides.
Learn more about:
hydrogen bonds
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