Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
37 Cards in this Set
- Front
- Back
|
First law of thermodynamics |
delta U= Q-W. Q= heat added to the system W= work done BY the system |
|
|
Adiabatic |
occurs when theres no heat exchange between the system and its environment. |
|
|
Isothermic does no work |
false |
|
|
isovolumetic does no work |
true |
|
|
Standard conditions |
measure of enthalpy, entropy, and Gibbs free energy. |
|
|
The temperature of the remaining water particles does not change as some of the high energy water particles get lost to vapor. True or False |
False |
|
|
What two factors facilitate condensation |
low temperature or high pressure. |
|
|
what is vapor pressure? |
when the gas particles of water apply pressure on the liquid at equilibrium. |
|
|
does vapor pressure decrease or increase with temp and why? |
It increases. The reason being is that as temp. goes up, kinetic energy goes up of those molecules and evaporate to the gaseous state. |
|
|
Boiling point |
the point at which vapor pressure of the liquid= ambient( atmospheric, applied, external pressure). |
|
|
sublimation |
when solid goes to gas. |
|
|
deposition |
from gas to solid. |
|
|
cold finger device and how it works |
1- heat up the solid at hot temp and low pressure 2-solid sublimes leaving impurities under 3-the gas then deposits on the colder finger. |
|
|
Phase diagrams |
graphs that show temperature and pressure at which a substance will be thermodynamically stable in a particular phase. They also show the temp and pressure at which phases will be in equilibrium. |
|
|
what do phase diagrams show |
substances' thermodynamically stable temp and pressure. -also pressure and temp for their equilibrium |
|
|
For the phase diagram, what are the general properties of the Liquid, gas, and solid. |
1- Gas= low pressure, high kinentic energy and therefore temp 2- Liquid= moderate for both. 3- Solid= Highly pressurized (therefore compact) and low temp. |
|
|
Temperature |
average kinetic energy of a substance |
|
|
Heat |
transfer of temperature (average kinetic energy) from one substance to another as a result of their difference of temperature. |
|
|
Zeroth law of thermodynamics |
objects are in thermal equilibrium only when their temps are equal |
|
|
First law of thermodynamics |
change in internal energy= amount of work transferred to a system- work done by a system |
|
|
how do you measure heat, q? whats the equation? |
q=MCAT LOL |
|
|
what is a heat capacity? |
product of mass and specific heat. |
|
|
When in phase change, we can not use the Q=MCAT, heat equation. We use enthalpy "H". |
true |
|
|
same formula used to calculate heat and phase changes. True or False |
FALSE. cuz no change in temp in phase change, so temp=0. |
|
|
whats the phase change formula. |
the phase change formula= Q=mass(m) x L (latent heat). |
|
|
for enthalpy, positive H is endothermic, negative H is exothermic. True or false |
true |
|
|
Hess's law |
enthlapy changes of a reaction are additive |
|
|
To calculate the enthlapy change for an equation that has both reactants and products. |
equation 7.6, in general chemistry. |
|
|
The equation for calculating entropy |
delta S= Q/temperature. |
|
|
How does entropy increase or decrease? |
when energy is distributed into a system the entropy increases. When energy is distributed out of a system (concentrated) the entropy decreases. |
|
|
Gibbs Free energy |
-it indicates whether a reaction will be spontaneous or not - Equation is delta G= delta H- T*delta S. GOLDFISH ARE HORRIBLE WITHOUT TARTAR SAUCE |
|
|
Exergonic Vs. exothermic? |
exergonic= gives off energy. Exothermic= gives off heat. |
|
|
Look at table 7.2 on page 232 of chemistry |
relationship between entropy, enthalpy and temp on Gibbs energy. |
|
|
Free energy of formation, delta G (subscript f). |
the free energy that occurs when 1 mole of a compound in its standard state is produced from its respective elements in their states under standard state conditions. |
|
|
Free energy of reaction |
delta G of rxn= sum of delta G formation of products- Sum of delta G formation of reactants.
|
|
|
Relationship between free energy and the equilibrium constant |
delta G of rxn= -RT ln Keq. The bigger the equilibrium constant, the bigger the natural log, more negative value of delta G and therefore its more spontaneous. |
|
|
The catalyst lower activation energy and free energy of reaction as well |
False, it only lowers activation energy |
