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How does vapor pressure of a substance depend on temperature and strength of intermolecular forces?
Wiki User
∙ 10y ago
As you increase a liquid's vapor pressure, you are decreasing the tendency of intermolecular forces to hold the particles of that liquid together. This is because as vapor pressure increases, the particles' kinetic energy increases. This means they move around more. The more they move around, the less ability the intermolecular forces have to bind them together. Eventually, when vapor pressure equals atmospheric pressure, boiling begins, and the intermolecular forces can no longer contain the liquid, and it becomes a vapor.
Wiki User
∙ 11y ago
Wiki User
∙ 12y agoThe stronger the intermolecular force, the more energy is required to boil the liquid, the higher the boiling point means the forces between molecules requires more energy to break and change the liquid to a gas.
Wiki User
∙ 11y agoYes.
The definition of a vapor pressure is the force the gas molecules are exerting in a liquid of a container. Gas particles start to exert pressure on the liquid when equilibrium is reached (Condensation &Vaporization happens at the same time). In a stronger intermolecular forces however, it is harder for vaporization to occur because it will take a lot of energy to break the bonds. Therefore, there will be less vapor pressure, in which fewer amount of gas molecules will exert a pressure on the liquid. In a weaker intermolecular force, it will be easier to break the liquid molecules into gas molecules so vapor pressure will be high. Just know that they are inversely related.
Wiki User
∙ 13y agoWeak intermolecular forces(of attraction). This means that the molecules are farther apart from each other. This makes the substance easier to evaporate.
Wiki User
∙ 13y agoHigh Surface tension
Low Vapor Pressure
High Boiling Point
Low Viscosity
Wiki User
∙ 10y agoDecreases with increasing intermolecular forces and increases with increasing temperature.
Wiki User
∙ 8y agoBoiling point is a property not a force; but a high boiling point indicate a strong intermolecular force.
Wiki User
∙ 11y agoNo, it is a strong inter-molecular force.
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How does intermolecular forces of a substance determine the phase the substance is in?
The strength of the intermolecular forces will determine what phase the substance is in at any given temperature and pressure. Consider the halogens for example, fluorine and chlorine are gases, while bromine is a liquid and iodine is a solid at room temperature. When considering the intermolecular forces present, each of these substances only has London forces, which increase in magnitude with increasing size of the molecules, and size increases as you go down a group in the periodic table. So, fluorine has the smallest intermolecular forces, and iodine has the largest. This explains why these different substances exist in different phases when at room temperature and pressure. The molecules in fluorine, for example, are only slightly attracted to each other, and therefore the substance exists as a gas. The stronger intermolecular forces in bromine, however, hold the molecules close to each other, but not quite strongly enough to prevent the molecules from sliding past each other; this makes bromine a liquid. Finally, in iodine, the intermolecular forces are actually strong enough that the molecules are held in fixed positions relative to each other, thus making iodine a solid.
What properties are affected by the strength of the intermolecular forces?
The physical properties of melting point, boiling point, vapor pressure, evaporation, viscosity, surface tension, and solubility are related to the strength of attractive forces between molecules.
What can you say about the relative strength of the intermolecular forces in the two compounds?
The intermolecular forces in acetone are weaker.
What is the relationship between the strength of the intermolecular forces and boiling point?
Boiling can only occur when the kinetic energy of heat overcomes the intermolecular forces holding a liquid together, so the greater the intermolecular forces, the higher the boiling point.
How do intermolecular forces compare to covalent and ionic bonds in terms of strength?
Ionic bonds create stronger intermolecular attraction than covalent bonds do; that is why rocks are harder than plastic.
How does intermolecular forces of a substance determine the phase the substance is in?
The strength of the intermolecular forces will determine what phase the substance is in at any given temperature and pressure. Consider the halogens for example, fluorine and chlorine are gases, while bromine is a liquid and iodine is a solid at room temperature. When considering the intermolecular forces present, each of these substances only has London forces, which increase in magnitude with increasing size of the molecules, and size increases as you go down a group in the periodic table. So, fluorine has the smallest intermolecular forces, and iodine has the largest. This explains why these different substances exist in different phases when at room temperature and pressure. The molecules in fluorine, for example, are only slightly attracted to each other, and therefore the substance exists as a gas. The stronger intermolecular forces in bromine, however, hold the molecules close to each other, but not quite strongly enough to prevent the molecules from sliding past each other; this makes bromine a liquid. Finally, in iodine, the intermolecular forces are actually strong enough that the molecules are held in fixed positions relative to each other, thus making iodine a solid.
The process by which particles move slowly enough for their attraction to bring them together to form a droplet of liquid?
The state of matter for any substance is dependent on the strength of their intermolecular forces as well as the temperature and pressure of the given system. When the temperature of a gas becomes lower than its unique boiling point, then it will become a liquid; called condensation.
What properties are affected by the strength of the intermolecular forces?
The physical properties of melting point, boiling point, vapor pressure, evaporation, viscosity, surface tension, and solubility are related to the strength of attractive forces between molecules.
How is pressure in the liquid related to depth?
Water pressure = height (depth) * density of substance * gravitational field strength
What causes the particles of a substance to be in one particular phase rather than another?
The phase of a substance is dependent on several things. Most basically, the composition of the substance itself and the strength of the atomic interactions within the substance determine how the other factors will effect it. For example, these interactions determine that water is liquid and steel is solid at room temperature. Substances changing phase depends on the temperature and the pressure exerted on them. The higher the temperature, the closer a substance gets to a gaseous phase. The lower the pressure, the same. This is the reason why water boils at a lower temperature if you are at a significantly higher elevation: there is less pressure. An interesting concept which has cool applications is that of a "triple point." Use Google to find a graphic image, so you can more easily figure out what I am saying. The triple point is the place at which the three phases meet, and each substance has its own triple point at a unique temperature and pressure. Below this point in temperature, pressure, or both, a substance will skip the liquid phase entirely and go directly from a solid to a gas, as in the case of "dry ice."
What can you say about the relative strength of the intermolecular forces in the two compounds?
The intermolecular forces in acetone are weaker.
What happens to strength when temperature of solid metal increases?
The pressure at which it yields is reduced as the temperature increases
What factor determine the strength of a rock?
The factors that influence the strength of a rock and how it will deform include temperature, confining pressure, rock type, and time.
What are the factors that influence the strength of a rock and how it will deform?
temperature, confining pressure, rock type, and time
Why alcohol evoporates?
Alcohols have intermolecular forces which are with relatively lower strength.
How does boiling point differ from normal boiling point?
The boiling point and normal boiling point are related concepts, but they have specific differences. Boiling Point: The boiling point of a substance is the temperature at which the vapor pressure of the liquid equals the atmospheric pressure, causing the liquid to change into a gas or vapor. At the boiling point, bubbles of vapor form within the liquid and rise to the surface, resulting in a continuous phase change from liquid to gas. Different substances have different boiling points, which can be influenced by factors such as atmospheric pressure and the strength of intermolecular forces within the liquid. Normal Boiling Point: The normal boiling point of a substance is the temperature at which it boils when the atmospheric pressure is at the standard pressure of 1 atmosphere (atm), which is equivalent to 101.325 kilopascals (kPa) or 760 millimeters of mercury (mmHg). This standard pressure is typically found at sea level.
Is the size of a molecule one factor in determining the strength of the intermolecular attractions?
Higher the size of the atom, it shows higher magnitudes of intermolecular compounds.
