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28 Cards in this Set
- Front
- Back
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Energy
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the capacity to do work or transfer heat
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Work
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the energy used to cause an object with mass to move against a force
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Heat
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the energy used to cause the temperature of an object to increase
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Kinetic energy
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energy of motion
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Potential energy
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the energy stored in an object or system due to its position in a force field or due to its configuration
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Force
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any kind of push or pull exerted on an object
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Kinetic Energy equation
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Ep=mgh
m=mass of object h=height of object relative to a reference height g=gravitational constant 9.8m/s^2 |
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electrostatic potential energy
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arises from interactions between charged particles
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electrostatic potential energy equation
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Eel = (kQ1Q2)/d
Q1, Q2: the electrical charges on two interacting objects d=the distance separating them K=constant of proportionality 8.99x10^9 J-m/C^2 opposites attract Eel < 0 < Eel like repel lower Eel=more stable |
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Chemical Energy
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potential energy stored in atomic arrangements
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Thermal energy
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energy a substance possesses due to its temperature
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Joule
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SI unit for energy
1 J = 1 kg-m^2/s^2 a mass of 2 kg moving at 1 m/s has Ek=1 J Ek=1/2 mv^2 = 1/2(2 kg)(1 m/s)^2=1 kg-m^2/s^2=1 J |
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Calorie
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non-SI
Obsolete: amount of energy required to raise the temperature of 1 g water from 14.5C to 15.5C Current: 1 cal = 4.184 J |
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System
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limited, well-defined portion of the universe singled out for study
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Surroundings
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Everything in the universe that is not the system
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Open System
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free exchange of matter & energy between system & surroundings
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Closed System
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energy may exchange between system & surroundings
matter may not exchange |
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Isolated System
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System cannot exchange energy or matter with surroundings
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Transfer of Energy
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w=F*d
work=Force*distance |
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first law of thermodynamics
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Energy is conserved, any energy lost by the system must be gained by the surroundings and vice versa
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internal energy
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sum of all Ek and Ep of all components
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internal energy equation
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ΔE=Ef - Ei
f=final i=initial |
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ΔE expressed
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sign, number, unit
+55 J energy lost to surroundings < 0 < energy gained from surroundings |
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ΔE related to heat & work
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ΔE=q+w
q=heat added to/liberated from system w=work done on/by system |
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Internal Energy Increase
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heat added to a system or work done on system
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Internal Energy Decrease
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heat liberated from a system or work done by a system
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Endothermic
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process of the system absorbing heat
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Exothermic
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process of the system losing heat
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