If conditions in the crankcase have become so bad that the oil pickup screen is clogged, you have more of a problem than just a clogged screen. If someone has poured sawdust or other trash into the crankcase you MIGHT be able to pull the pan and clean the screen. If it's clogged for any other reason, you'll need to rebuild the engine.
If you have crankcase pressure in an engine, it's because your crankcase ventilation system has become clogged. There is a hose running from your valve cover to your air intake; this gets clogged up with oil. Pull it out, clean it in solvent, blow through the hose to make sure you can, and put the car back together.
vapor pressure of a pure solvent is the pressure needed for the gas to escape the pure solvent in vapor form. its partial pressure in this case will be the pressure of that escaped vapour (in the mixture of air). in simpler terms vapor pressure describes a single condensable system (just the vapor of the solvent and the liquid state of the solvent) while its partial pressure describes the multicomponent system (air). they are essentially the same thing describing different systems
Solubility is the ability of a solute to dissolve in a solvent at a certain temperature and pressure.
When one adds a solute to a solvent, several properties of the solvent change. This include the boiling point, the freezing point, the vapor pressure and the osmotic pressure.
The solute is carbon dioxide gas under pressure; the solvent is water.
the solute is carbon dioxide gas under pressure and the solvent is water.
A nonvolatile ( not readily evaporated) solute elevates the boiling point of a solvent (the temperature at which the solvent boils) because its presence lowers the vapor pressure of the solvent. * The normal boiling point of a liquid occurs at the temperature where the vapor pressure is equal to 1 atmosphere. * The presence of a nonvolatile solute decreases the number of solvent molecules per unit volume , so less molecules escape form the liquid. Thus the vapor pressure of the solvent decreases. * Therefore, such a solution with lower vapor pressure must be heated to a higher temperature than the boiling point of the pure solvent to reach a vapor pressure of 1 atmosphere.
The addition of a non-volatile solute decreases the vapor pressure of the solution compared to the pure solvent. The decrease in vapor pressure is related to the mole fraction of the solvent in the solution, as shown by Rauolt's Law. This happens primarily because the solvent molecules are involved in interactions with the solute particles. The effect on boiling point is pretty simple. The boiling point is the temperature where the vapor pressure of the solution equals atmospheric pressure. If the vapor pressure of the solution is lower than the solvent, then a higher temperature will be required to raise the vapor pressure of the solution to its boiling point. The effect on solutes on the freezing point of the solution mainly has to do with entropy. The entropy of the solvent in a solution is higher than the entropy of the same pure solvent.
The vapor pressure of 1 m sucrose (C12H22O11) is higher than the vapor pressure of 1 m NaCl where the solvent is water Sea water has a lower vapor pressure than distilled water. The vapor pressure of 0.5 m NaNO3 is the same as the vapor pressure of 0.5 m KBr, assuming that the solvent in each case is water The vapor pressure of 0.10 m KCl is the same as the vapor pressure of 0.05 m AlCl3 assuming the solvent in each case is water The vapor pressure of 1 m NaCl is lower than the vapor pressure of 0.5 m KNO3, assuming that the solvent in each case is water The vapor pressure of 0.10 m NaCl is lower than the vapor pressure of 0.05 m MgCl2 assuming the solvent in each case is water.
Temperature, pressure, the amount of the solute surface area exposed to the solvent and the saturation point of the solvent are some of the factors.
Solute, lower (apex)
A solution has a higher vapor pressure than a pure solvent. This is why salt water boils faster than pure water.
the temperature and the pressure at which the solute is dissolved in a solvent.
Solvent molecules moving across a selectively-permeable membrane into an area of lower solvent concentration.
temperature, pressure, presence of other chemical species (for the same solute and the same solvent)
There are fewer solvent molecules at the surface that can evaporate.
The solubility of a gas in a solvent is directly proportional to the partial pressure of that gas above the solvent.
It becomes heavier. The movement of solvent through a membrane produces a pressure called the osmotic pressure. This happens when the pressure in which the solvent is flowing is raised to the equivalent of the pressure moving through the membrane from the hypotonic side.
by adding solvent, the ability of solvent molecules to escape(i.e its vapour pressure) will decrease.because the solute particles provide hinderance
- temperature - pressure - stirring - dimension of the solid particles - nature of the solvent and the nature of the solid material - an additive in the solvent
Examples are: temperature, ratio solute/solvent, pressure, stirring, surface area of the solvent.
the nature of the solute and solvent, temperature and pressure