Term
| What are the states of matter? |
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Definition
| Gas(g),Liquid(l),Solid(s) |
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Term
| What are the properties of the Gas state(g)? |
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Definition
Indefinite shape
Indefinite volume
Particles widely seperated
Particles moving rapidly |
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Term
| What are the properties of the Liquid state(l)? |
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Definition
indefinte shape
fixed volume
particles in close contact
particles can move past one another |
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Term
| What are the properties of the Solid state(s)? |
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Definition
fixed shape
fixed volume
particles in close contact
particles vibrate around a central position |
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Term
| What is the kenetic theory of gases? |
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Definition
Theory that a gas contains small particles in constant random motion that have no attractive or repulsive forces between them or the walls of the container, are very far apart from each other with a very small negligible total volume compared to the container it occupys,
and has an average kinetic energy proportional to absolute temperature |
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Term
| How does kinetic molecular theory of gases explain why gases have low density? |
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Definition
| since gases are spread out and have little mass per unit of volume causes them to have a low density |
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Term
| How does kinetic molecular theory of gases explain why gases are highly compressible? |
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Definition
| since total gas volume is small and the particles are far apart, the container volume can be reduced considerably and still leave space between the gas particles |
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Term
| How does kinetic molecular theory of gases explain why gases have no definite shape or volume? |
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Definition
| because gases are in constant, random motion and therefore reach all parts of any container they are in |
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Term
| How does kinetic molecular theory of gases explain why gases diffuse? |
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Definition
| since gas particles are in constant,random motion. if the container is opened the gas particles move out into the surrondings |
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Term
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Definition
| spontaneous movement from a region of high partial pressure to a region of low partial pressure. |
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Term
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Definition
| Force exerted per unit of area |
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Term
| What is the equation for pressure? |
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Definition
P(Pressure)=F(Force)
A(Area)
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Term
| What is the equation for Kinetic Energy? |
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Definition
| KE(Kinetic Energy)=1/2M(mass)*V2(velocity) |
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Term
| What is the average KE(Kinetic Energy) proportional to? |
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Definition
| AVG KE is directly proportional to T(Temperature) |
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Term
| How does the Kinetic Moleculat Theory of Gases explain why gases never settle? |
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Definition
| since there is no attraction or repulsion between gas particles no net energy is lost when particles come in contact with each other or the container. this also explains why the travel in straight lines between collisions. |
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Term
| 1 atm(atmosphere)=How many Torr, and mmHG? |
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Definition
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Term
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Definition
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Term
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Definition
| Device used to measeure atmospheric pressure |
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Term
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Definition
| A device used to measure gas pressure inside a reaction vessel |
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Term
| What is Boyle's Law(Pressure-Volume Law)? |
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Definition
at a constant amount of gas at a constant temperature
V(Volume) is inversely related to P(Pressure) |
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Term
| What is the Pressure-Volume Law equation? |
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Definition
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Term
| What is Charles's Law(Volume-Temperature Law)? |
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Definition
For a fixed (constant) amount of gas at a constant pressure
T(Temperature) is directly proportional to V(Volume) |
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Term
| What is the Volume-Temperature Law equation? |
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Definition
V1/T1=V2/T2
Temperature must be in Kelvin
K=°C+273
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Term
| What is the Combined Gas Law equation? |
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Definition
P1V1/T1=P2V2/T2
Moles stay constant and Temperature in K(Kelvin) |
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Term
| What is Avogadro's Hypothesis? |
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Definition
| When two gases are at the same temperature and pressure then equal volumes of the gases will contain equal number of particles(moles) |
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Term
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Definition
Standard temperature and Pressure
Standard temp= 0°C or 273K
Standard Pressure= 1 atm or 760 torr
At STP the volume occupied by 1 mol of any gas is 22.4L
22.4L/mol is the standard molar volume of a gas |
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Term
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Definition
| a gas that obeys all the gas laws under all conditions |
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Term
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Definition
| a gas that deviates from ideal behavior at high pressures and low temperatures |
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Term
| What is the Ideal Gas Law equation? |
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Definition
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Term
| What is the equation for molar mass? |
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Definition
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Term
| What is partial pressure? |
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Definition
| The pressure a gas in a mixture would exert if it were the only gas in the container. |
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Term
| What is Dalton's Law of Partial Pressure? |
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Definition
| The total pressure of a mixture of gases is equal to the sum of the partial pressures of all gases in the mixture |
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Term
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Definition
| the partial pressure of the gas phase(vapor) of a substance over a sample of the liquid phase of the substance at equilibrium |
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Term
| What is mole fraction(X)? |
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Definition
the moles of a substance in a mixture compared to the total moles in the mixture.
Can be expressed
XA= nA = PA
nT PT |
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Term
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Definition
| diffusion through a small hole. |
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Term
| What is Graham's Law of Effusion? |
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Definition
the rate of effusion of a gas is inversely proportional to the square root of the density of the gas.
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Term
| Heavier gases effuse more what? |
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Definition
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Term
| Lighter gases effuse more what? |
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Definition
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Term
| Effusion rate is also proportional to? |
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Definition
| 1/Square root of molar mass |
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Term
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Definition
| the study of the energy changes that occur in chemical reactions |
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Term
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Definition
| The study of heat, work, and energy in general and its transformations. |
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Term
| What is the definition of exothermic? |
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Definition
| Chemical reactions that produce heat |
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Term
| What is the definition of endothermic? |
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Definition
| Chemical reactions that absorb heat |
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Term
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Definition
| The capacity to do work or transfer heat |
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Term
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Definition
The energy of motion.
KE=1/2m(mass)V2(velocity) |
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Term
| What is potential energy? |
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Definition
| Stored energy related to an objects position or composition |
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Term
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Definition
| energy used to change the motion of an object? |
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Term
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Definition
| Energy transferred from a hotter object to a cooler one |
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Term
| What is temperature proportional to? |
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Definition
heat but is not the same as heat energy.
EX: Bucket of warm water has more heat energy than a match because it has more mass |
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Term
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Definition
| Object, reaction, or process you are studying. |
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Term
| What are the surrondings? |
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Definition
| Everything else outiside a system |
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Term
| What is the first law of thermodynamics? |
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Definition
| Energy cannot be created or destroyed it can only move from one place to another or transform into another form of energy |
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Term
| What is the internal energy equation? |
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Definition
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Term
| Heat and work energy flowing into the system is what? |
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Definition
| a positive quantitity in respect to the system |
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Term
| Heat and work energy flowing out of the system is what? |
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Definition
| A negative quantity in respect to the system |
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Term
| What is the PV work function? |
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Definition
| w=-P(pressure)ΔV(change in volume) |
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Term
| What is a state function? |
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Definition
| any quantity whose value is independent of the pathway taken to get that quantity |
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Term
| Are heat and work state functions? |
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Definition
| No because their values depend on how the system loses heat or does work. |
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Term
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Definition
The internal energy(E) plus Pressure X Volume
H=E+PV |
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Term
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Definition
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Term
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Definition
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Term
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Definition
| Measuring of heat flows for processes |
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Term
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Definition
| the amount of heat needed to raise the temperature of a substance or object by one degree celsius or one kelvin unit |
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Term
| What is molar heat capacity? |
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Definition
| the amount of heat needed to raise the temperature of one mole by one degree celsius or one kelvin unit |
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Term
| What is specific heat capacity? |
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Definition
| the amount of heat needed to raise the temperature of one gram of substance by one degree celsius or one kelvin unit |
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Term
| What is the calorimetry equation? |
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Definition
| q= m(mass)X Cs(specific heat)X ΔT(Change in Temperature) |
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Term
| What is heat or enthalpy of fusion? |
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Definition
| The energy needed to melt a substance |
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Term
| What is heat or ethalpy of vaporization? |
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Definition
| the energy needed to vaporize a substance |
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Term
| What is the heat equations for the flat segments on a Heating and Cooling Curve? |
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Definition
q=ΔHfus X moles
q=ΔHvap X moles |
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Term
| What is the heat equations for the slope segments on a Heating and Cooling Curves? |
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Definition
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Term
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Definition
| Spontaneous change from liquid to gas at any temperature |
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Term
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Definition
| Rapid formation of gas bubbles within a liquid |
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Term
| What is the boiling point? |
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Definition
| point at which the liquid and gas states are at equlibrium. |
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Term
| What is the normal boiling point? |
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Definition
| temperature at which liquid and gas are at equlibrium at 1 atm of pressure |
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Term
| What is the normal melting point? |
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Definition
| Temperature in which solid and liquid states are at equilibrium under 1 atm of pressure. |
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Term
| What is the triple point? |
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Definition
| temperature and pressure at which gas, liquid, and solid phases of a substance are all at equilibrium. |
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Term
| What is the critical point? |
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Definition
| temperature and pressure above which the distinction between gas and liquid dissapears. |
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Term
| What is the critical temperature? |
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Definition
| temperature above which a substance can no longer exist as a liquid regardless of any external pressure |
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Term
| What is the critical pressure? |
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Definition
| external pressure needed to keep a substance in the liquid state at the critical temperature |
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Term
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Definition
| phase transition of a solid directly to a gas |
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Term
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Definition
| Phase transition of a gas directly to a solid |
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Term
|
Definition
| Phase transition of a gas to a liquid |
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