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Thermochemistry Flashcards

Thermochemistry

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976213940EnergyThe capacity to do work. Its formula is =q (heat) +w (work)
976213941WorkThe result of a force acting through distance and its formula is =-P∆V
976213942HeatFlow of energy caused by a temperature difference and its formulas =m×Cs×∆T or E+PV
976213943Kinetic EnergyEnergy of motion.
976213944Potential EnergyEnergy associated with position or composition chemical energy.
976213945Law of Conservation of EnergyEnergy can neither be created or destroyed→transferred.
976213946Kinetic Energy FormulaKE=1/2mv²
976213947Joule Formula1 kgm²/v²
976213948CalorieOriginally defined as the amount of energy require to raise the T of 1 g of H₂0 by 1°C.
9762139491,000 calorieHow many calories are in 1 Calorie?
9762139501st Law of ThermodynamicsThe total energy of the universe is constant.
976213951Internal Energy (E)The sum of the kinetic and potential energies of all of the particles that compose the system.
976213952The current stateWhat does the value of a state function depend on?
976213953Work and heatWhat are two things that are not state functions because it matters how they got there?
976213954It is gained by the surroundingsWhat happens to energy lost by the system?
976213955EnergyWhat can be exchanged with heat and work?
976213956Heat CapacityThe quantity of heat required to change the T by 1°C.
976213957Molar Capacityraise the T of mole by 1°C.
976213958Pressure-volume workWhen the force is caused by a volume change against an external pressure.
976213959CalorimetryMeasure of the thermal energy of reaction (system) by observing ∆T of the surroundings.
976213960Bomb CalorimeterUsed for combustion reactions.
976213961EnthalpyThe sum of a systems internal energy and the product of its pressure and volume. (H)
1017809201endothermicThe sign for an __________ reaction has a positive ∆H and absorbs heat from the surroundings; feels cold to touch.
1017809202exothermicThe sign for an __________ reaction has a negative ∆H and gives off heat to the surroundings; feels warm to touch.
1017809203extensive propertyEnthalpy for a reaction of heat is an ___________.
1017809204multipliedIf a chemical equation is ___________ through by some factor the ∆Hrxn is also multiplied by some factor.
1017809205signIf a chemical reaction is reversed, the ∆Hrxn changes _____.
1017809206sumIf a chemical reaction can be expressed as the sum of a series of steps, then ∆Hrxn for the overall equation is the ____ of the heats of reactions for each step.
1017809207gasesThe standard state for _______ is pure gas at pressure of exactly of 1 atm.
1017809208liquids or solidsThe standard state for _________ the pure substance is in its most stable form at a pressure of atm and T of interest (usually 25°C).
1017809209enthalpy changeThe standard ________ ________ is ∆H° is the change in enthalpy for a process when all reactants and products are in their STD states.
1017809210pure compoundThe standard enthalpy of formation ∆Hf° for a ______ __________ is the change in enthalpy when 1 mole of the compound forms from its constituent elements in their STD states.
1017809211compoundThe standard enthalpy for a pure _______ in its STD state is ∆Hf°=0.
1017809212standard heat of formation∆Hf° is also called...
1017809213losesAs the system (+) gains thermal energy, the system ______ (-) energy.
1017809214losesAs work is done on the system (+), the system done by the system ______ energy.
1017809215flows, outAs energy ______ into the system, energy flows _____ of the system.
1017809216volume, negativeAs ______ increases, work is done on the surroundings, so work should be ________.
1023889556state functionInternal energy is a ______ _______, which means its value depends only on the state of the system, now on how the system arrived at that state.
1023889557intensiveSpecific heat capacity and molar heat capacity are ________ properties-they depend on the kind of substance being heated, not the amount.

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