part 2
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| viscosity | resistance of a liquid to flow
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| the greater the viscosity the (blank) it flows | the slowly it flows
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| how do you measure viscosity | how long a liquid takes to flow out of a pipette under the forces of gravity. How fast an object sings through the liquid.
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| what does viscosity measure? | the ease that molecules move past one another
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| how are viscosity and T related? | inversely proportional. Viscosity decreases with increasing T. The increasing kinetic energy overcomes the attractive forces and molecules can move easily past each other
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| What happen to the molecules in the interior of the liquid? | they experience an attractive force from neighboring molecules which surround on all sides
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| what happens to the molecules at the surface of a liquid? | molecules on the surface have neighboring molecules only on one side (the side facing the interior) and thus experience an attractive force whic pull them into the interior
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| surface tension | the energy required to increase the surface area of a liquid
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| water surface tension at 20 C | 7.29 * 10^ -2 J/m^2
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| cohesive forces | bind molecules of the same type together
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| adhesive forces | bind a substance to a surface
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| "capillary" action | water move up a thin capillary against the force of gravity
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| phase changes | matter in one state changes to another state
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| sublimation | solid changes to gas
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| melting (fusion) | solid changes to liquid
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| freezing | liquid changes to solid
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| vaporization | liquid changes to gas
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| condensation | gas changes to liquid
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| deposition | gas changes to solid
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| fusion | the melting process for a solid
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| heat of fusion (triangle H sub fus) | the enthalpy change associated with melting a solid
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| ice heat of fusion = ? | 6.01 kJ/mol
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| heat of vaporization (triangle H sub vap) | heat needed for the vaporization of a liquid
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| water heat of vaporization = ? | 40.67 kJ/mol
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| true or false: less energy is needed to allow molecules to move past each other than to separate them totally | true
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| True or false: great energy is needed to vaporize water than to melt it | true
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| specific heat/molar heat capacity | the amount of heat needed to change the T of a substance
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| specific heat of ice | 2.09 J/gK
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| specific heat of water | 4.18 J/gK
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| specific heat of water vapor | 1.84 J/gK
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| how can gases be liquified? | by decreasing the T or increasing the P
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| Is it easier or harder to use P to liquify gas as T increase? | harder (due to increasing kinetic energy)
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| critical temperature | the highest T at which a substance can exist as a liquid
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| critical pressure | the pressure required to bring about condensation at the critical T
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| is melting, sublimation, and vaporization exothermic or endothermic processes? | endothermic processes
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