Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Chemistry
Thermodynamics
| Term | Definition |
|---|---|
| Kinetic Energy Equation | KE=1/2mv^2 |
| First Law of Thermodynamics | Energy of Universe is Constant |
| Second Law of Thermodynamics | For any Spontaneous Process, the entropy of the universe increases |
| Third Law of Thermodynamics | The entropy of a perfect crystal at absolute temperature is Zero |
| dE=q+w | q=heat energy (MCdT) w=work energy (-PdV) |
| Specific Heat Capacity | Heat required to raise temp of 1 gram of substance by 1 degree C |
| Molar Heat Capacity | Heat required to raise temp of 1 mole of substance by 1 degree C |
| Calculate quantity of heat released or absorbed | q=MCdT |
| Calculate Work W=-PdV | dV = volume, P=external pressure |
| ΔH = ΔE + PΔV | change in enthalpy/heat |
| If ΔH > 0? | Endothermic |
| if ΔH < 0? | Exothermic |
| Standard enthalpy change | ΔHProducts - ΔHReactants |
| Particles-most freedom to least freedom | Translational, Rotational, Vibrational |
| Gases can be condensed by | Decreasing temperature or increasing pressure |
| A reaction is spontaneous if | ΔG < 0 (Entropy of universe increases) |
| Standard Enthalpy Change for a reaction | ΔSrxn = Sproducts Sreactants |
| Free Energy Changes in Chemical Reactions | ΔGrxn = ΔHrxn TΔSrxn |
Created by:
tubaman300
Popular Chemistry sets