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| 5135820081 | Different forms of energy | potential or kinetic. Potential energy comes in forms that are stored including — chemical, gravitational, mechanical, and nuclear. Kinetic energy forms are doing work — like electrical, heat, light, motion, and sound. | 0 | |
| 5135822163 | Units in which energy is expressed | 1 cal = 4.184 J 1 J = 1 km m2 / s2 | 1 | |
| 5135824756 | First law of thermodynamics | The law of conservation of energy states that the total energy of an isolated system is constant; energy can be transformed from one form to another, but cannot be created or destroyed. | 2 | |
| 5135831233 | How is the change of internal energy related to the exchanges of heat and word between a system and its surrounding? | 3 | ||
| 5135833838 | State function and its importance to themodynamics | 4 | ||
| 5135833839 | Enthalpy | a thermodynamic quantity equivalent to the total heat content of a system. It is equal to the internal energy of the system plus the product of pressure and volume. the change in enthalpy associated with a particular chemical process. H=E+PV | 5 | |
| 5135836985 | Enthalpy Diagram | Endo +++++ |  | 6 |
| 5137095704 | Enthalpy Diagram | Exo ------ | 7 | |
| 5135836986 | Heat Capasity | the number of heat units needed to raise the temperature of a body by one degree. | 8 | |
| 5137101607 | Internal energy | the change in internal energy, ΔE, is the final energy of the system minus the initial energy of the system: ΔE = Efinal − Einitial | 9 | |
| 5135839707 | Specific heat | the heat required to raise the temperature of the unit mass of a given substance by a given amount (usually one degree). | 10 | |
| 5137115235 | For q - means... + means... | + system gains heat - system loses heat | 11 | |
| 5137116796 | For w - means... + means... | + work done on system - work done by system | 12 | |
| 5135843611 | Hess's Law | states that regardless of the multiple stages or steps of a reaction, the total enthalpy change for the reaction is the sum of all changes. This law is a manifestation that enthalpy is a state | 13 | |
| 5135845832 | Standard State | the change in enthalpy when one mole of a substance in the standard state (1 atm of pressure and 298.15 K) is formed from its pure elements under the same conditions. | 14 | |
| 5135848535 | Standard states for C, H, & O | C = 0 H = gas O = gas | 15 | |
| 5135850899 | Standard heat of formation and which chemical reaction? | The standard enthalpy of formation or standard heat of formation of a compound is the change of enthalpy during the formation of 1 mole of the compound from its constituent elements, with all substances in their standard states at 1 atmosphere (1 atm or 101.3 kPa). =heat transferred/mass change | 16 | |
| 5137683876 | Specific heat for water | 4.184 J/g-K | 17 | |
| 5137061095 | Is work a state function? Why or why not? | No, it doesn't produce heat | 18 | |
| 5137063858 | What is an example of state function? | 19 | ||
| 5137631032 | Work equation | w = -PΔV | 20 |
