chem unit 6
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Last updated 1:09 PM on 5/9/23
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44 Terms
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adiabatic
a process that occurs without transfer of heat or matter between a thermodynamic system and its surroundings.
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boiling point
the temperature in which the vapor pressure of the liquid is equal to external or atmospheric pressure.
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calorie
the amount of energy needed to raise the temperature of one gram of water by one degree Celsius.
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calorimetry
experimental determination of the enthalpy changes of reactions.
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celcius
a temperature scale defined by the freezing and boiling points of pure water as 0 o C and 100 o C.
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change of state
a substance going from solid to liquid, liquid to gas or the reverse of those processes.
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condensation
the movement of molecules from the gas phase to the liquid phase.
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dietary calorie
a unit used to determine the amount of energy in foods which is equal to 1 kilocalorie.
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endothermic
a thermodynamic process in which heat flows into the system from the surroundings.
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energy
the capacity to do work and transfer heat.
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enthalpy
the amount of heat energy gained or lost by a process at constant pressure.
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enthalpy of fusion
the heat energy required to convert a solid to a liquid at the melting point.
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enthalpy of a solution
the amount of heat gained or lost in the process of solution formation.
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enthalpy of vaporization
the amount of heat energy required to convert a liquid to gas at the boiling point.
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entropy
the measure of the degree of randomness and disorder in the system.
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exothermic
a thermodynamic process in which heat flows from the system to the surroundings.
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fahrenheit
a temperature scale defined by the freezing point and boiling point of pure water to be 32 o F and 212 o F.
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first law of thermodynamics
the total energy in the universe is constant.
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fusion
the state change from solid to liquid.
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hess’s law
Heat evolved in a reaction can be calculated by adding heats measured from other reactions (sum of all enthalpy changes).
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internal energy
the sum of the potential and kinetic energies of particles in a system.
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isothermal
a change of a system in which the temperature remains constant.
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joule
the SI unit of energy.
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kelvin
a temperature scale in which the units are the same size as Celsius degrees but the zero point is the lowest possible temperature or absolute zero.
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kilocalorie
a unit of energy equivalent to 1000 calories.
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kilojoule
a unit of energy equal to 1000 Joules.
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kinetic molecular theory
all matter is made up of a large number of small particles that are in constant random motion.
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law of conservation of energy
the overall energy in the universe is constant.
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melting point
the temperature at which the crystal lattice of a solid collapses and the solid starts to convert to liquid.
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second law of thermodynamics
the overall entropy of the universe increases with every spontaneous reaction.
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specific heat capacity
the quantity of heat necessary to change the temperature of 1 gram of any substance by 1 o C or 1 K.
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standard enthalpy of a reaction
the enthalpy change that occurs from a reaction with all reactants and products in their standard states.
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standard molar enthalpy of formation
the enthalpy change for the formation of 1 mole of a compound directly from its elements in their standard states.
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standard state
the most stable form of an element or compound in the physical state at 1 bar of pressure and a specified temperature.
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sublimation
the direct conversion of a solid to a gas with no liquid phase.
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surroundings
everything outside of the system in a thermodynamic process.
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system
the collection of objects or substances being evaluated in a thermodynamic process.
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temperature
a physical property that determines the direction of heat flow in an object or a measure of its average kinetic energy.
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thermal equilibrium
a condition in which the system and surroundings are at the same temperature and heat transfer stops.
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thermodynamics
the science of heat and work.
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triple point
the temperature and pressure at which the solid, liquid and gas phases of a substance are in equilibrium.
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vaporization
the state change from a liquid to a gas.
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volatility
the tendency of the molecules of a liquid to escape into the gas phase.
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work
quantity of energy transferred by a force acting through a distance.
Note 
Flashcards (24)