in brief...
- molecules of methane are bonded by dispersion forces
- dispersion forces are the weakest form of intermolecular bonding, meaning that there is only a small amount of energy (or heat) required to break the weak dispersion forces between the methane molecules
- because there is not much heat required to break dispersion forces - we can understand why methane boils so easily and at such a low temperature
[explanation of dispersion forces in more detail...
- electrons inside an atom move around the nucleus randomly
- it is likely that, at any one instant, there may be more electrons on one side of the nucleus than the other
- this results in one side of the atom being more negatively charged than the other at this instant (the side with more electrons on it than the other would obviously be more negatively charged)
- now to explain how this applies to intermolecular bonding...well - to make things easier, I'll name one molecule BOB and another STEVE. imagine that STEVE is standing to BOB's left. if say, we froze time - and at that instant there were more electrons on the left hand side of BOB's body - the left hand side of BOB would become negatively charged. the electrons inside STEVE (who is standing to BOB's left) would suddenly be repelled to his left, as far away from the negative side of BOB as possible. thus the right hand side of STEVE would become positively charged while the left hand side of STEVE would become negatively charged just like BOB. this would continue on in a domino kind of a way to surrounding molecules - and the attraction between the negatively charged side of BOB and the positively charged side of STEVE is what we call dispersion forces.
in more scientific terms: dispersion forces are the attraction that exists between molecules because of the temporary dipoles (differences in charge of one side of a molecule to the other) that form as electrons move randomly
- dispersion forces are very, very weak - which explains why molecules that are bonded in this form have such low boiling temperatures]
The vapor density of an equimolar mixture of methane (CH4) and oxygen (O2) would be the average of the individual vapor densities of methane and oxygen. The vapor density of methane is approximately 8 g/L and oxygen is approximately 16 g/L, so the equimolar mixture would have a vapor density close to 12 g/L.
The vapor pressure graph shows that as temperature increases, the vapor pressure also increases. This indicates a direct relationship between temperature and vapor pressure, where higher temperatures result in higher vapor pressures.
The saturated vapor pressure of water at 50 oC is 123,39 mm Hg.
The vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature. The vapor pressure depends on the temperature and the substance.
The vapor pressure vs temperature graph shows that as temperature increases, the vapor pressure also increases. This indicates that there is a direct relationship between vapor pressure and temperature, where higher temperatures lead to higher vapor pressures.
The vapor pressure deficit formula is used to calculate the difference between the actual vapor pressure and the saturation vapor pressure in the atmosphere. It is calculated by subtracting the actual vapor pressure from the saturation vapor pressure.
Ozone, Methane, Water vapor.
The vapor density of an equimolar mixture of methane (CH4) and oxygen (O2) would be the average of the individual vapor densities of methane and oxygen. The vapor density of methane is approximately 8 g/L and oxygen is approximately 16 g/L, so the equimolar mixture would have a vapor density close to 12 g/L.
The vapor pressure graph shows that as temperature increases, the vapor pressure also increases. This indicates a direct relationship between temperature and vapor pressure, where higher temperatures result in higher vapor pressures.
To calculate the vapor pressure deficit (VPD), subtract the actual vapor pressure (e) from the saturation vapor pressure (es) at a given temperature. The actual vapor pressure can be calculated using the relative humidity (RH) and the saturation vapor pressure can be determined from the temperature. The formula is VPD es - e, where es saturation vapor pressure and e actual vapor pressure.
The saturated vapor pressure of water at 50 oC is 123,39 mm Hg.
The vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature. The vapor pressure depends on the temperature and the substance.
To determine the actual vapor pressure of a substance, one can use a device called a vapor pressure thermometer. This device measures the pressure exerted by the vapor of the substance at a specific temperature. By comparing the vapor pressure readings at different temperatures, one can determine the actual vapor pressure of the substance.
The vapor pressure vs temperature graph shows that as temperature increases, the vapor pressure also increases. This indicates that there is a direct relationship between vapor pressure and temperature, where higher temperatures lead to higher vapor pressures.
True Vapor Pressure is the pressure of the vapor in equilibrium with the liquid at 100 F (it is equal to the bubble point pressure at 100 F)
Vapor pressure deficit (VPD) is calculated by subtracting the actual vapor pressure (e) from the saturation vapor pressure (es) at a given temperature. The formula for VPD is VPD es - e.
Mainly ammonia, methane, and water vapor.