Term
| what is a system and surroundings in thermodynamic problems |
|
Definition
| a system is the macroscopic body under study, and the surroundings are everything else |
|
|
Term
| what are the three systems of thermodynamic classification |
|
Definition
| open, closed and isolated |
|
|
Term
|
Definition
| open systems exchange both mass and energy with it's surroundings |
|
|
Term
| what do closed systems exchange |
|
Definition
| closed systems exchange energy but not mass with their surroundings |
|
|
Term
| what do isolated systems exchange |
|
Definition
| isolated systems do not exchange either mass or energy with its surroundings |
|
|
Term
|
Definition
| such properties that describe the state of a system |
|
|
Term
| there are only two ways to transfer energy between systems, what are they |
|
Definition
|
|
Term
|
Definition
| the natural transfer of energy from a warmer body to a cooler body |
|
|
Term
|
Definition
| any transfer of energy that is not heat |
|
|
Term
| what are the three forms of heat |
|
Definition
| conduction, convection and radiation |
|
|
Term
|
Definition
| thermal energy transfer via molecular collisions |
|
|
Term
| give an example of conduction |
|
Definition
| when higher energy molecules transfer some of its energy to lower energy molecules via molecular collision |
|
|
Term
|
Definition
| differences in pressure and density drive warm fluid to cooler fluid |
|
|
Term
|
Definition
| thermal energy transfer via electromagnetic waves- when a metal is heated it glows bright orange and then blue- this is electromagnetic waves |
|
|
Term
| what is Newton's law of cooling |
|
Definition
| the cooling of a body is directly proportional to the temperature difference betweenthe body and its environment |
|
|
Term
| in constant pressure conditions, how can you calculate the work being done |
|
Definition
|
|
Term
| how can you find the average kinetic energy of a single molecule in any fluid |
|
Definition
|
|
Term
| what is change in enthalpy |
|
Definition
| delta H= delta U + PdeltaV |
|
|
Term
| An element in its standard state at 25 C is arbitrarily assigned |
|
Definition
|
|
Term
| for reactions involving no change in pressure, the enthalpy equals |
|
Definition
| the enthalpy equals the heat |
|
|
Term
| when there is an absence of work within a reaction |
|
Definition
| the enthalpy is equal to the change in energy |
|
|
Term
| what is the heat of the reaction |
|
Definition
| this is the change in heat from the reactants to products |
|
|
Term
| what does endothermic mean |
|
Definition
| the enthalpy change is positive |
|
|
Term
| what does exothermic mean |
|
Definition
| the enthalpy change is negative |
|
|
Term
| what sort of chemical state does the activation energy hill represent |
|
Definition
| it represents the transitional state |
|
|
Term
| a catalyst affects the what but not the what |
|
Definition
| it affects the rate but not the equilibrium |
|
|
Term
|
Definition
| this is the tendancy toward disorder |
|
|
Term
| something with higher entropy has higher |
|
Definition
|
|
Term
| what does the second law of thermodynamics state |
|
Definition
| that entropy of an isolated sysytem will never decrease |
|
|
Term
| only reactions equal to zero are considered ideal reactions and only ideal reactions have |
|
Definition
|
|
Term
| what dictates the direction of a reaction |
|
Definition
|
|
Term
| reactions at equilibrium have achieved |
|
Definition
| the maximum universal entropy |
|
|
Term
| when temperature, volume and pressure increase, so does |
|
Definition
|
|
Term
| when is zero entropy applied |
|
Definition
| with any pure substance or any molecule at absolute zero |
|
|
Term
| a negative delta G indicates |
|
Definition
|
|
