Energy and Heat
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| energy | power which may be translated into motion, overcoming resistance, or effecting physical change; the ability to do work. Symbol E
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| work | energy used to move an object against an opposing force
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| kinetic energy | energy of motion 1/2 mass x volume squared
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| potential energy | Potential energy is that energy which an object has because of its position
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| law of conservation of energy | first law of thermodynamics-energy cannot be created nor destroyed, just transferred
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| system and surroundings | when energy flows into a system from the surroundings, the system gains energy(from/into/loses)
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| heat | transfer of thermal energy between system and surroundings
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| heat capacity | amount of heat required to raise one mole of substance by one degree Celsius
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| specific heat | amount of heat per unit mass required to raise one mole of substance by one degree Celsius
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| first law of thermodynamics | Law of conservation of energy-energy cannot be created nor destroyed, just transferred
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| bond energy | amount of energy required to break a covalent bond
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| exothermic | loss of energy delta E is -
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| endothermic | gain in energy delta E is +
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| calorimeter | container designed to create an isolated system, so that heat measurements can be carefully made(either constant-volume or constant-pressure)
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| enthalpy | delta H-heat for a process under constant pressure conditions
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| delta H = | delta E + P(delta V)
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| P x V = | n x R x T
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| heat of solution | energy released or required to dissolve a specific quantity of a a given substance in water
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| heat of dilution | energy released or required to dilute an existing solution
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| Molar Heat of Fusion | energy required to melt one mole of a given substance
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| Molar Heat of Vaporization | energy required to evaporate one mole of a given substance
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| standard heat of formation | delta Hf- delta Hrxn to create 1 mole of product from its elements in their standard states
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| Hess' Law of heat summation | the overall heat gain/loss in a chemical process equals the sums of the enthalpy changes in each step of the process(delta Htot=delta H1 + delta H2 + ...)
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| molar energy change | (delta Emolar)change in energy for a process that involves one mole of a given material
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| work = | -external pressure x change in volume
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| change in energy of the system equal | system heat plus system work
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| change in energy of the universe | change in energy of the system plus the change in energy of the surroundings which equals zero
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| measurement for energy | joule(J)=1 N m=1 kg m squared/seconds squared
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| 1 L atm | 101.325 joules
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| 1 calorie | 4.184 Joules
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| 1 Cal | 1 kcal
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| 1st Step in calculating energy change using a calorimeter | take measurements of the mass of the material and before temperature
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| 2nd Step in calculating energy change using a calorimeter | mix chemical reagents being studies directly in the calorimeter and measure after temperature
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| 3rd Step in calculating energy change using a calorimeter | calculate where change in energy(delta q)=mass of the solution(m) x change in temperature(delta t) x specific heat of the solution(water=1.00 cal/gC or 4.185 J/gC)
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| reaction energy(delta Hrxn)= | sum of bond energies broken - sum of bond energies formed
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Created by:
elainero
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