A decrease in temperature will affect vapor pressure by: increasing the density of the gas molecules, thus making them heavier and more difficult to move around decreasing the surface area of the gas molecules, thus decreasing the number of collisions occurring increasing the rate of condensation decreasing the average kinetic energy of the molecules, making them move slower and collide less

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A decrease in temperature will affect vapor pressure by: increasing the density of the gas molecules, thus making them heavier and more difficult to move around decreasing the surface area of the gas molecules, thus decreasing the number of collisions occurring increasing the rate of condensation decreasing the average kinetic energy of the molecules, making them move slower and collide less

Chemistry
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Temperature = average kinetic energy of your particles. Average kinetic energy = how fast your particles move. If you lower the temperature the particles will move more slowly and intermolecular forces will become more significant. Vapor pressure has to do with liquids. When we raise the temperature the vapor pressure goes up because more particles can make it into the gas phase. If we lower the temperature the particles don't move around as quickly and fewer can escape and become vapor. Remember vapor pressure depends on the temperature and also how strong your IMF are and whether there are solvent molecules in your solute. The vapor pressure rises until it reaches the external pressure and when that happens you get boiling.
Would it be the last one?
I think it's the last one

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To me surface area makes no sense

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