Textbook Chapter 5
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bomb calorimeter
device designed to measure the energy change for processes occurring under conditions of constant volume, commonly used for reactions involving solid and gaseous reacts or products
calorie
unit of heat or energy, amount of energy required to raise 1 gram of water by 1 degree celcius (4.184 J)
calorimeter
device used to measure the amount of heat absorbed or released in a chemical or physical process
calorimetry
process of measuring the amount of heat involved in a chemical or physical process
chemical thermodynamics
area of science dealing with relationship between heat, work, and all forms of energy associated with chemical and physical processes
endothermic process
chemical reaction or physical change that absorbs heat
energy
capacity to supply heat or do work
enthalpy (H)
sum of a systems internal energy and the mathematical prodcut of its pressure and volume
enthalpy change (/_\H)
heat released or absorbed by a system under constant pressure during a chemical or physical process
exothermic process
chemic reaction or physical change releasing heat
expansion work (pressure-volume work)
work done as a system expands or contracts against external pressure
first law of thermodynamics
internal energy of a system changes due to heat flow in or out of system and work done on or by system
heat (q)
transfer of thermal energy between 2 bodies
heat capacity (c)
extensive property of a body of matter representing the quantity of heat required to increase tempreature by 1 degree C
Hess’s law
process can be represented as the sum of several steps and the enthalpy change of the process equals the sum of the enthalpy changes of hte steps
hydrocarbon
compound composed of hydrogen and carbon, makes up most fossil fuels
internal energy (U)
total of all possible kinds of energy present in a substance or substances
joule (J)
Si unit of energy
kinetic energy
energy of a moving body, in joules, equal to 1/2mv^2 (m=mass, v=velocity)
potential energy
energy of particle or system of particles derived from relative position, composition, or condition
specific heat capacity (c)
intensive property of a substance that represents quantity of heat required to raise temp of 1 g by 1 C
standard enthaly of combustion (/_\Hc)
heat released when one mole of a compound undergoes complete combusion under standard conditions
standard enthalpy of formation (/_\Hf)
enthalpy change of chemical reaction which 1 mole of pure substance is formed from its elements in their most stable states under standard conditions
standard state
set of physical conditions as accepted as common reference conditions for reporting thermodynamic properties