| Question | Answer |
| The branch of science that studies the transfer of energy during chemical reactions or phase changes | Thermochemistry |
| The AVERAGE KINETIC energy in the particles of a sample | temperature |
| measures the TOTAL amount of thermal energy transferred from one object to another | Heat (expressed in Joules) |
| It is _________ to determine the absolute amount of heat in something | impossible |
| Chemists measure the _________ in energy that occurs during a chemical reaction | change |
| Is the heat content of a system at a constant pressure | Enthalpy (H) |
| An insulated container, similar to a thermos, in which a thermometer detects the temperature change that occurs during a chemical reaction | Calorimeter |
| A Calorimeter measures ________ | Enthalpy |
| Produces a temperature change (you can sense it happening | sensible heat |
| produces a phase change - FLAT on the graph - no change is detected | Latent heat |
| The amount of heat that has to be added to overcome the intermolecular forces so a solid can MELT | Molar enthalpy of fusion |
| The amount of heat required to convert a mole of a liquid at its boiling point to its vapor at the same temperature | Molar enthalpy of vaporization |
| The amount of energy that raises 1g of something by 1 degree C | Specific heat |
| High Specific Heat | LARGE amounts of heat |
| High specific heat retains heat values for ______ periods | longer |
| Low Specific Heat | Small amounts o energy |
| the change on enthalpy that occurs during a reaction is called the | enthalpy of reaction (delta H) |
| A chemical equation that shows the reactants, products, and amount of energy that is released or absorbed as heat | Thermochemical equation |
| Reverse reactions have the same magnitude, but _________ signs | different |
| Standard state | 25 degree C and 1 atm |
| is the enhalpy change that makes 1 mole in its standard state from its elements in their standard states | Standard molar enthalpy of formation |
| The energy released as eat by the complete burning of one mole of a substance in standard conditions | Enthalpy of combustion |
| Combustion reactions must contain ________ | oxygen |
| EXothermic | heat EXits |
| The enthalpy change of a reaction equals the sum of the enthalpy changes for each step of the process | Hess's Law |
| Chemical bonds _____ energy | STORE |
| When bonds are broken, energy is _______ | RELEASED |
| Bonds are broken through ________ | VIBRATION |
| The strength of the bond between any two atoms depends on the ________that are bonding and on the _________of the bond | Elements / length |
| Bonded atoms are ________ ________ than unbonded ones | more stable |
| Energy is __________ ___________ to break bonds | ALWAYS REQUIRED |
| Bond breaking is thus always an __________ process | ENDOTHERMIC |
| Forming bonds is always an ________ process. | EXOTHERMIC |
| The ______ the bond, the MORE energy is released | STRONGER |
| A reaction that breaks strong bonds and forms weak ones __________ energy | REQUIRES |
| A reaction that breaks weak bonds and forms strong ones _________ energy | RELEASES |
| In most cases, exothermic processes are thermodynamically _______ | favorable |
| Ice melting, compressed gas is released and gets colder | Examples of endothermic reactions |
| Things are going from order to _____ | disorder |
| Entropy is a measure of _________ | RaNdomNeSS |
| Entropy increases with ______ | temperature |
| Entropy is theoretically equal to zero at ________ ________ | absolute zero |
| ____ processes increase the entropy of the universe | All |
| A negative delta S tries to go against the tendency of disorder and attempts to _______ ___ | decrease it |
| - H + S | -G at all Temps |
| -H -S | -G at low temps |
| +H +S | -G at high temps |
| +H -S | +G at all temps |
| Formulated a single way of figuring out favorability | J. Willard Gibbs |
| Gibbs combined entropy and enthalpy into a single term called_____ ______ | Free Energy |
| -delta G is ___________ | SPONTANEOUS! (Like you know who...negative and may spontaneous try to kill you_ |
