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30 Cards in this Set
- Front
- Back
Energy
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the ability to do work
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Work
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the force applied to an object times the distance that the object travels parallel to that force
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Heat
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energy that is transferred as a consequence of temperature differences
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Hypothesis
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an educated guess explaining observations
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Theory
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a hypothesis that has been tested by experiments
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Scientific law
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a theory that has been confirmed by many experiments
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The first Law of Thermodynamics
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energy cannot be created or destroyed
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Potential energy
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energy that is stored
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Kinetic energy
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energy that is in motion
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Joule
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metric unit for energy that lifts 102g 1 meter
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Calibration
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the process of using certain physical measurements to define the scale of a measuring device
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0.0 C or 32.0 F
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the temperature of any mixture of ice and water
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100.0 C or 212.0 F
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the temperature of any boiling water
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C = 5/9(F-32)
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equation for calculating Celsius
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F = 9/5(C) + 32
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equation for calculating Fahrenheit
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Kelvin
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absolute temperature scale
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K = C + 273.15
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equation for calculating Kelvin
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1 calorie
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the amount of heat necessary to warm one gram of water one degree Celsius
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1 calorie = 4.184 Joules
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relationship between calories and joules
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1 food calorie (Cal) = 1,000 chemistry calories (cal)
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relationship between Cal and cal
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Heat Capacity (or specific heat)
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the amount of heat necessary to raise the temperature of 1 gram of a substance by 1 degree Celsius
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Calorimetry
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the process used to measure heat
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Experimental scatter
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The reflection that all measurements have some inacurasies .
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Heating curve
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A graph showing how a substance's phases (gas, liquid or solid) changes while being heated.
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Heat capacity formula
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q = mc∆T
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Delta T formula
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∆T = T(final) - T(initial)
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Heat capacity units
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J/g°C or cal/g°C or cal/kg°C
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Specific heat of water
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1.000 cal/g°C or 4.184 J/g°C
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Calibrate a thermometer
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Note the reading at the temp of ice/water mixture and apply the difference between the reading and the actual tempreture of freezing to future measurements.
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Calorimetry equation
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-q(object) = q(water) + q(calorimeter)
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