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Chem. Chapter 6
vocab for Ch. 6
| Question | Answer |
|---|---|
| energy | the ability to do work or transfer heat: energy= work + heat |
| work | energy used to cause an object that has mass to move |
| heat | evergy used to cause temperature of an object to rise |
| potential energy | energy an pbject posseses by virtue of its position of chemical composition |
| kinetic energy | energy an object posesses by its motion: KE= 1/2 mv^2 |
| chemical energy | the energy stored within bonds of chemical substances |
| radiant energy | comes form the sun and is earth's primary energy source |
| thermal energy | energy associated with the random motion of atoms and molecules: proportional to Kelvin |
| nuclear energy | energy stored within the collection neutrons and protons in the atom |
| thermodynamics | study of heat and its transformations |
| thermochemistry | branch of thermodynamics that deals with thte heat involved with physical and chemical changes |
| fundamental premise | when energy is transferred from one object to another it apears as work and or as heat |
| system | composed of particles with their own internal energies (E or U) |
| internal energy | of a system, that is the sum of all kinetic and potential energies of all components of a system (E) |
| heat 2 | energy can also be transferred as heat: flows from warmer objects to cooler objects |
| thermochemistry | a study of heat change in chemical reactions: this can be endo- or exo- |
| heat 3 | the transfer of thermal energy between two bodies that are at differenct temperatures |
| temperature | the measure of the thermal energy |
| First Law of thermodynamics | energy is niether created nor destroyed: energy of the universe is constant: if system loses energy must be gained by surroundings and vice versa |
| pressure | force per unit area |
| state function | internal energy of a system is independent of the path by which the system achieved that state |
| enthalpy | heat of a reaction, the internal energy plus the product of pressure and volume |
| enthalpies of chemical change | heats of a reaction; amount of heat exchanged per mole of a substance produced |
| exothermic | heat flows out of the sytem into the surroundings and change of H is a negative sign |
| endothermic | heat flows into the system from surroundings and change of H is a positive sign |
| calorimetry | science of measuring heat changes (q) for chemical reactions |
| bomb calorimetry | measures the heat change at constant volume such that q= change in E |
| constant pressure calorimetry | measures the heat change at constant pressure such that q= change in H |
| heat capacity | amount of heat required to raise the temperature of an object or substance one degree C or K |
| specific heat | amount of heat required to raise one gram of substance by one degree C |
| molar heat | amount of heat required to raise the temperature of 1 mole of substance 1 degree |
| Hess's law | overall enthalpy change for one reaction is equal to the sum of the enthalpy changes for the individual steps in the reaction |
| standard heat of formation | enthalpy change for the formation of one mole of substance in standard state from its constituent element |
| thermodynamic standad states | most stable form of a substance at one atm and 25 degrees C and one molar concentration for all |
Created by:
dee_roberts_1223
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