whathappen to the boiling point of alkanes if they were under higher pressure?
472294
As a general rule boiling point of substances increase with increase in pressure.\n\nAlkanes of smaller no. of carbon atoms are gases at NTP but if pressure is increased the alkanes will convert to liquids.\n\nAll isomers of Butane (4 C atoms) and Propane (3 C atoms) will easily convert to liquids at high pressure.\nThe role of temperature in converting gases to liquids will be of prime importance.\n\nHigh alkanes under high pressure will gradually become more and more viscuss.
822453
The boiling point series for short alcohols is dominated by hydrogen bonding.  That's where the H on the hydroxyl group (OH)  on one molecule is attracted to the O on a nearby molecule.\nEven tough "normal alcohol" (I imagine you mean n-butanol from the context of your question) is just as heavy, it will have a higher boiling point because its structure makes hydrogen bonding easier.  It is basically alike to a bunch of strings with the magnets on their ends with nothing to impede the other strings from glomming on.\nTert-butanol, on the other hand, is like a bunch of knotted strings with magnets at the base of the knot.  The hydroxyl group on these molecules are not all that available for their neighboring molecules to find and be attracted to.  This is called "steric hinderance" and is more a physical and spatial consideration than a chemical phenomenon.
297778
the higher alkanes, liquid from pentane up, have poisonous effects as solvents. they interfere with the nervous system and can be used to get a "high"
455047
r u really serious !!! how can one find a pie bond in an alkane????
7988
hydrogen bonds will increase the boiling point of a substance, all else being equal.\none way to see this is by looking at the boiling point of alcohols.\nthere is a near linear correlation between length fo the carbon chain and the boiling point for straight chain carbohydrate alcohols. as the chain gets shorter, the boiling point goes up faster than the linear relation would suggest, until you get to water  where hydrogen bonding is the most active and the boiling point jumps dramatically.
195312
Are you seriously a 4th grader...^\n\nProbably because the liquid may be slightly impure and the only way to get the true boiling point of the liquid is to measure the temperature at the reflux ring.
849983
low pressure = lower boiling point = lower dew point
730844
OK...You can start with the equation of DG (I'm using D instead of writing "delta").\n\nDG = DH -TDS  You've seen that equation, right?  OK..Since the boiling point of water is 100 degreed C at 1 atm pressure, we are really talking about an equilibrium situation.  So, DG= 0.\n\nConsequently, DH = TDS.  \n\nSince you know DH and you know T (in Kelvin), you can calculate DS.  Make sure that you convert DH into Joules (instead of kilojoules) before you finish the problem.
427695
To "boil" something means to heat it to its boiling point and (I guess ) watch bubbles form and pop.  "Boiling point" means the temperature at which a substance turns from liquid to gas (this temperature will depend on the air pressure or pressure of another gas on the liquid: no pressure means no liquid phase).\n\nWe're used to thinking of water doing this as it turns from liquid to gas, but any liquid turning into a gas at the right temp will do it. So start with liquid nitrogen, heat it, watch bubbles form.  The liquid is nitrogen in liquid phase; the bubbles are nitrogen in gas phase.  It's still just nitrogen (N2, two atoms of nitrogen stuck together to make a single molecule).  The N2 bubbles burst and the nitrogen floats away, that's all.  By the way, this happens at -170 degrees or so, as I recall, so don't touch it....hard to think of this as "boiling" temperature, but there it is......
78161
I'm not sure that is true. If by 'thickness' you mean viscosity, then there are some liquids that are more viscous than water that boil at much lower temperatures. For example, ethanol has a viscosity of 1.074 × 10-3 Pa*s  and boils at 78 degrees C. Water has a viscosity of 0.890 × 10-3 Pa*s and boils at 100 C. The boiling point of a liquid is really more dependent on the amount of energy needed to overcome various types of molecular bonding, that vary with the liquid, such as dipole-dipole, induced-dipole, and hydrogen bonds.\n\nThe density of a liquid has no relation to its boiling point. A good example is olive oil and water. Olive oil has a boiling point of 570 degrees F., yet floats on water because it is less dense.
968042
Boiling is vapour pressure phenomenon. A liquid always exerts a pressure in the space just above it due to evaporation of its surface molecule which is called vapor pressure of that particular liquid and as temperature is raised the vapour pressure goes on increasing. When vapor pressure of the liquid exceeds atmospheric pressure liquid starts to boil.\nin case of a mixture, the solute molecules bind the molecules of the solvent and thus there are fewer surface molecule available to evaporate from the liquid surface. Due to which vapour pressure exerted by a mixture is always less than vapor pressure of pure solvent. To make vapor pressure of mixture to reach the atmospheric pressure level its temperature should be raised more than temperature of solvent alone. Thats why a mixutre has a boiling point elevation.
879801
Pentane\n\nIt depends on which compound has the strongest intermolecular forces. In the case of hydrocarbons the intermolecular forces that are present are dispersion forces.\nIn such cases:\n"The more branched a molecule is, the more "spherical" it is, and the smaller surface area it will have - since dispersion forces increase with surface area, the more branched molecules will have a lower boiling point. You may notice that the trend in the melting points is rather different - this is because the longer a branch is, the more potential it has to flop around and disrupt the regular crystalline lattice of frozen pentane, giving a liquid state."
649941
The boiling point of water is dependant on the (air) pressure on it. Put water into a pressure cooker and its boiling point will increase. Take water to the bottom of a deep mine and the BP will be above 100 degrees. Theoretically. the boiling point in the centre of a cyclone would be lower than in the centre of a high pressure cell.\n\nThe atmospheric pressure on the surface of the water is what stops water molecules escaping. The lower the pressure the easier it is for them to escape and the higher the pressure the harder it is for these molecules to escape. The boiling is the violent action of the molecules trying to escape.
317634
Pressure will increase if temperature increases, assuming that the container remains at a constant volume. Because the molecules are moving faster, they collide more often with the walls of the container, so the pressure goes up.\n\nThis is demonstrated by Gay-Lussac's Law, which states that that for a fixed amount of gas (fixed number of moles) at a fixed volume, the pressure is proportional to the temperature, so:  P/T = constant.\n\nIn case you need to know this for a test, and easy mnemonic  is "Pete and Tom are Gay" (Pressure and Temperature are proportional according to Gay-Lussac).
444782
Phosphine, arsine, and ammonia are all gases at ambient temperature and pressure.  But ammonia has a higher boiling point than the other 2, about -33 C.  All 3 are polar molecules.  But ammonia can form hydrogen bonds.  This increases the strength of the intermolecular forces, causing the liquid state to be more stable.
1187079
Boiling point depends on the strength of the intermolecular forces. Following is the list of them all with their strength and when they occur. \nnetwork covalent (strongest) with only diamond or SiO2\nIonic (ionic compound, 2nd strongest) like Na-Cl etc. Gets stronger with smaller sizes. \nHydrogen bonding (N, O, F with H) 3 rd strongest. \nDipole dipole (when there is a polar molecule) 4 th strongest, gets stronger with more polarity. \nLondon dispersion weakest. Stronger with more mass. \n\na NH3of the first two. Because NH3 has hydrogen bonding (only if you have N, O, or F with hydrogen) while PH3 has regular dipole dipole (based on polarity), which is weaker than NH3. \nNow in this one its c because if you draw their Lewis diagrams out c molecule has on O----H bond while d doesn't. That hydrogen bond is strong enough to make c stronger. As other than that they only have London dispersion force, (which are found in non polar molecules, and they get stronger as atomic mass gets higher). \ne and f both have the London dispersion force that I talked about earlier cause they both are non polar. So f has greater mass so f has higher boiling point. \ng because HCl has polarity (dipole dipole forces) which are stronger than F2 which is non polar and has London dispersion forces (they are the weakest).
854658
I'm assuming that you mean refined petroleum because you would have had more detail if it was a specific oil.\nThe answer is negative 150 degrees Fahrenheit