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Chemistry I Chap 8
Vocab
| Term | Definition |
|---|---|
| Conservation of Energy Law | AKA first law of Thermodynamics; energy can be neither created nor destroyed. Thus, the total energy of an isolated system is constant |
| Endothermic | A reaction in which heat is absorbed and the temperature of the surroundings falls |
| Energy | The capacity to do work or supply heat |
| Enthalpy (H) | The quantity E + PV |
| Enthalpy Change (^H) | The heat change in a reaction or process at constant pressure ^H = ^E + P^V |
| Entropy (S) | The amount of molecular randomness in a system |
| Exothermic | A reaction in which heat is evolved and the temperature of the surroundings rises |
| First Law of Thermodynamics | The total internal energy of an isolated system is constant |
| Gibbs Free-Energy Change (^G) | ^G=^H-T^S |
| Heat | The energy transferred from one object to another as the result of a temperature difference between them |
| Heat Capacity (C) | The amount of heat required to raise the temperature of an object or substance a given amount |
| Heat of Combustion (^H'c) | The amount of energy released on burning a substance |
| Heat of Reaction (^H) | The enthalpy change for a reaction ^H |
| Hess's Law | The overall enthalpy change for a reaction is equal to the sum of the enthalpy changes for the individual steps in the reaction. |
| Internal Energy (E) | The sum of kinetic and potential energies for each particle in a system |
| Joule (J) | The SI unit of energy, equal to 1 (kg*m^2)/s^2 |
| Kinetic Energy (Ek) | The energy of motion Ek=(1/2)mv^2 |
| Molar Heat Capacity (Cm) | The amount of heat necessary to raise the temperature of 1 mol of a substance 1'c |
| Potential Energy (Ep) | Energy that is stored, either in an object because of its position or in a molecule because of its chemical composition |
| Specific Heat | The amount of heat necessary to raise the temperature of 1 gram of a substance 1'c |
| Spontaneous Process | One that proceeds on its own without any continuous external influence |
| Standard Enthalpy of Reaction (^H') | Enthalpy change under standard-state conditions |
| Standard of Heat Formation (^H'f) | The enthalpy change ^H'f for the hypothetical formation of 1 mol of substance in its standard state form from the most stable forms of its constituent elements in their standard states |
| State Function | A function or property whose value depends only on the present condition of the system, not on the path used to arrive at that condition |
| Sublimination | The direct converstion of a solid to a vapor without going through a liquid state. |
| Temperature | A measure of the kinetic energy of molecular motion. |
| Thermochemistry | A study of the heat changes that take place during reactions. |
| Thermodynamic Standard State | Conditions under which thermodynamic measurements are reported 298.15 K (25'c) 1 atm pressure for each gas 1 M concentration for solutions |
| Work (w) | The distance (d) moved times the force (F) that opposes the motion W=d*F |
Created by:
fenlien
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