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plain on a particle basis why the vapor pressure of a solution is lower than a pure solvent.
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Hello Today we’ll be talking about Chapter 14 Question 42 which asks us to consider the difference in the vapor pressure between a pure liquid and a solution and, more importantly, to explain on a particle level. Why, exactly? The vapor pressure decreases when we have a solution with dissolved particles. So if we have our pure liquid here we have some water. Here’s a water molecule, and here is another water molecule. And here’s our vapor pressure where we have gaseous water. That’s above Thea couple. And in this case, the water has an equilibrium where the water breaks all of the ah inter molecular interactions that it might have and is able to leave as a gas floats away. We break these inter molecular hydrogen bonds and float away. However dissolved is a solution where we have dissolved particles. I’m gonna draw slightly bigger cup. Here’s our water. We have our same water molecules, and we have There’s another one, and they have the same inter molecular interactions and so on. However, I’m actually gonna make this cup a little bit larger. Let’s say we added some an A c e o sodium chloride. Now, in addition, to this sort of interaction between water molecules. We also have water molecules. They’re interacting with the actual cat. I owns sodium. And so we have bonds here, more bonds to all the sodium because this is how they’re salivated. And similarly, we have chlorine here, which has similar interactions with Thea Hydrogen Sze and so overall, their arm or bonds that have to be broken toe. Let a water molecule go free into the gas. And so because there are more bonds in the ah, here’s the pure liquid. And here’s the solution. Their arm, or inter molecular between molecules Maur inter molecular bonds to break in a solution, because you need to break not only the bonds between the water molecules themselves, which are present in both but in the solution. You also need to break the bonds between the water molecules and the salyut, so water and sodium and water in chlorine, and thus it’s less favorable to break all those bonds. And so you have a lower vapor pressure, less water is able to escape. Hopefully, this enters some of your questions about how the collective property of vapor pressure is affected on the particle level by dissolving salutes in a solution
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Frequently Asked Questions About explain on a particle basis why the vapor
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Why does a solution containing a nonvolatile solute have a lower vapor pressure than a pure solvent?
The vapor pressure of the solution is lower than the vapor pressure of the pure solvent because the solute particles do not evaporate.
Why does a solution’s vapor pressure differ from a pure solvent’s vapor pressure?
The solution is thermodynamically more stable than a pure solvent because fewer molecules are evaporating into the gas phase as a result of the stability of the solution, which results in a lower vapor pressure.
Why does adding a non-volatile solute cause the vapor pressure of a solution to drop?
This is because the surface area is partially occupied by solvent molecules and partially by nonvolatile solute molecules, which lowers the rate of evaporation.
Why does the vapor pressure drop as intermolecular forces rise?
Strong intermolecular forces cause fewer molecules to have enough kinetic energy to escape at a given temperature, so these substances will have lower vapor pressure. Substances with high vapor pressures are said to be volatile, meaning they easily evaporate.
Does higher volatility imply a lower vapor pressure?
When describing volatility, vapor pressures or boiling points (for liquids) are frequently used; high vapor pressures denote high volatility, while high boiling points denote low volatility.
What is the relationship between the vapor pressure of the nonvolatile substance and it?
The vapour pressure of a non-volatile solute solution is equal to the mole fraction of the pure solvent’s vapour pressure at that temperature.
What connection exists between the vapor pressures of the solvent and the solution?
According to the formula psolution = xApsolvent, or Raoult’s law, the vapor pressure of a solvent in a solution is equal to its mole fraction times its vapor pressure as a pure liquid.
Why does vapour pressure differ from water’s?
Solution: Since glucose is a non-volatile solute, its molecules won’t condense into vapours, resulting in a lower vapour pressure than water, which is why the vapour pressure of a solution of glucose in water is lower than that of water.
What changes do the more solute particles there are to the vapor pressure?
The vapor pressure of the solvent decreases as more solute is dissolved in it, and this causes the vapor pressure of the solvent to change more over time.
What causes the vapor pressure to drop as the temperature drops?
Temperature: A higher temperature allows for more molecules to have enough energy to escape from a liquid or solid, while a lower temperature allows for fewer molecules to have enough energy to do so.
What connection exists between intermolecular forces of attraction and vapor pressure?
The strength of the intermolecular forces between the molecules of a liquid determines its vapor pressure; the stronger these forces, the slower the rate of evaporation and lower the vapor pressure.
What elevates the vapor pressure?
When a liquid in a closed container is heated, more molecules escape the liquid phase and evaporate; as a result, there is an increase in vapor pressure because more vapor molecules are colliding with the container walls more frequently.
What elements influence the vapor pressure?
Surface area, molecule type, and temperature are some of the factors that affect a liquid’s vapour pressure. If the temperature rises, the vapour pressure also rises; conversely, if the temperature falls, the vapour pressure decreases.
What factors affect vapor pressure?
The vapor pressure of a liquid does not change depending on how much liquid is present in the container, whether it is one liter or thirty liters; both samples will have the same vapor pressure at the same temperature.
What causes vapor pressure?
When a liquid is heated, its molecules gain enough kinetic energy to overcome the forces keeping them in the liquid and they escape into the gaseous phase, creating a population of molecules in the vapor phase above the liquid, which results in a pressure, the vapor pressure of the liquid.
What has the biggest impact on vapor pressure?
The most significant factor that affects vapor pressure is temperature because it increases the kinetic energy of molecules, which speeds up their escape from a liquid at higher temperatures. This increases vapor pressure.