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co2
The intermolecular forces are stronger in solids.
The covalent bond is an intramolecular bond.An example of compound having covalent bonds is carbon dioxide - CO2.
Gasses are compressible and liquids and solids are incompressible. Using this information one can surmise that CO2 compressible would be the gas phase of CO2 and CO2 incompressible would be the solid (dry ice) phase of CO2.
Burning combines Carbon and Oxygen gas from organic materia. The resulting CO2 molecules are more stable, that is, less energy, because they are stronger.
intermolecular force between the sio2 molecule is greater than that of the co2 molecule....the co2 molecule is in it gaseous state while that of the sio2 is crystalline making the intermolecular force stronger than that of the co2 molecule.
co2
The intermolecular forces are stronger in solids.
NO2 has a higher boiling point than CO2 because the nitrogen radii is larger than carbon. The bigger the atom the more intermolecular force that is created...this requires more energy to break causing a higher boiling point.
The covalent bond is an intramolecular bond.An example of compound having covalent bonds is carbon dioxide - CO2.
KCl is an ionic substance (strong intermolecular forces) and CO2 is a non-polar covalent substance (weak intermolecular forces)
Of CO2, CS2 and CSe2, CO2 is the smallest molecule whereas CSe2 is the largest molecule. The same pattern exists in the strength of the intermolecular forces. All three are linear, non polar molecules.
Induced dipole best describes why molecules like CF3CF3 are soluble in liquid CO2.
High vapor pressure and low intermolecular forces
increasing the CO2 concentration in the atmosphere
Increasing the CO2 concentration in the atmosphere
The cause is the pressure difference between the gas pressure in the bottle and the atmospheric pressure.