Heating Curve Turk.

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Presentation transcript:

Heating Curve Turk

Energy is absorbed Energy is released

Potential Energy- stored energy Kinetic Energy- energy having to do with motion

Heat of Fusion amount of heat needed to be absorbed to convert a unit of mass of a substance from a solid to a liquid at its melting point q= mHf heat of fusion for water is 334 joules per gram. Example: How many joules are required to melt 255 g of ice at 0 C at 1 atm?

Heat of Vaporization amount of heat needed to be absorbed to convert a unit mass of a substance from its liquid phase to gas phase. q = Hvm heat of vaporization for water is 2260 joules per gram. Example: How many joules of energy are required to vaporize 423 g of water at 100 C and 1 atm?

Heating Curve for Water vaporization E gas D 100 condensation C liquid melting Temperature (oC) Melting, freezing, vaporization, condensation, sublimation, and deposition are six common phase changes. Note: The temperature of a substance does not change during a phase change. B A freezing solid Heat added LeMay Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World , 1996, page 487

Heating Curve Temperature of the ice (solid) is increasing; increase in temperature means an increase in kinetic energy. At 0oC the ice begins to melt. During melting, the temperature stays the same; there is no change in kinetic energy. There is a change in potential energy; potential energy is increasing. The temperature of the water now rises from 0oC to 100oC.

Heating Curve 4. At 100oC, the water boils (changes to gas). When the water boils, the temperature stays the same; no change in kinetic energy. There is a change in potential energy; potential energy increases. 5. After all the water boils, the temperature of the gas rises.