O2 because it has more electrons. Because of the higher number of electrons, it has higher dispersion forces (attractive forces). This means that more energy (heat) is required to unstick the molecules into a different state of matter.
LOx (liquid diatomic oxygen) boils at -182.96oC, -297.33oF.
NaCl has the highest boiling point. It is an ionic compound with strong bonds between sodium and chlorine ions, requiring more energy to break these bonds and reach the boiling point compared to the other substances listed.
The boiling point in degree Celsius are given below:Na: 883K: 774Si: 2355Ne: -246Silicon has the highest boiling point among the elements given.
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.
It isn't even a gas at that temperature let alone being ideal. The boiling point of O2 is 90 K and the melting point is 55K. So at 33 K it is a solid. At extremely low pressures this might change a bit, but you gave a huge pressure so not the case.
a) O2 would have a higher boiling point than N2 since it experiences London dispersion forces in addition to its higher molecular weight. b) SO2 would have a higher boiling point than CO2 due to its ability to form stronger dipole-dipole interactions and London dispersion forces. c) HF would have a higher boiling point than HI due to hydrogen bonding, which is stronger than the dipole-dipole interactions present in HI.
LOx (liquid diatomic oxygen) boils at -182.96oC, -297.33oF.
The atoms in O2 move much too quickly to boil. ;D
NaCl has the highest boiling point. It is an ionic compound with strong bonds between sodium and chlorine ions, requiring more energy to break these bonds and reach the boiling point compared to the other substances listed.
HF is electronegative compared to O2. HF has delta plus and delta minus creating a dipole moment, it is a polar molecule therefore it has a higher boiling point. O2 which is symmetrical and non polar (looks like O=O) and therefore has no dipole moment.
The boiling point in degree Celsius are given below:Na: 883K: 774Si: 2355Ne: -246Silicon has the highest boiling point among the elements given.
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.
It is simply the water that freexes. Water is not simply a mixture if hydrogen and oxygen. The two elements are bound together to form water molecules. So it must be treated as its own substance. The behavior of water cannot be explained using the behavior of elemental hydrogen or oxygen. Its properties are different from its constituent elements.
It isn't even a gas at that temperature let alone being ideal. The boiling point of O2 is 90 K and the melting point is 55K. So at 33 K it is a solid. At extremely low pressures this might change a bit, but you gave a huge pressure so not the case.
Melting point 54.36 K (-218.79 °C, -361.82 °F) Boiling point 90.20 K (-182.95 °C, -297.31 °F) Critical point 154.59 K, 5.043 MPa Heat of fusion (O2) 0.444 kJ·mol−1 Heat of vaporization (O2) 6.82 kJ·mol−1 Specific heat capacity (25 °C) (O2) 29.378 J·mol−1·K−1
Helium and oxygen can be separated using cryogenic distillation. Since helium has a lower boiling point (-268.9°C) compared to oxygen (-183°C), they can be separated by cooling the mixture to a temperature between their respective boiling points and then distilling them off as separate components.
Common results point to "You can not clean an O2 sensor, it must be replaced"