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47 Cards in this Set
- Front
- Back
____ phase is a separate phase from liquid water
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Aqueous
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Systems may have several ____ and ____ phases, but typically only one ____ phase exists for a given system
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liquid
solid gas |
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____ - A measure of the energy necessary to change the temperature of the substance in a given phase by 1 degree Celsius
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Heat capacity
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____ is a process the transfer of energy, a process cannot be stored
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Heat
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A process where there is no heat flow is called an ____.`
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adiabatic process
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Work is ____, so when gas does work on the surroundings it is transferring energy to the surroundings
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energy transfer
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Average kinetic energy = 3/2 RT applies here, the gas gets ____ when the molecules move ____
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hotter
faster |
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A constant ____ heat capacity is greater than a constant ____ heat capacity (for a gas)
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pressure
volume |
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For liquids and solids increase in potential energy as the molecules move apart, that is because energy increases when objects that are ____ to each other are ____.
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attracted
separated |
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C=
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C= Q/ΔT
C = Heat capacity Q = heat flow ΔT = change in temperature (This formula assumes that all the energy transferred is heat) |
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Work must also be considered as a form of ____
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energy transfer
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____ - temperature change expressed per unit mass
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Specific heat
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Q=
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Q= mcΔT
M = mass of the substance c = the specific heat of the substance |
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____ is for an entire system, specific heat is per mass of a substance
Can even have molar or volume ____ which is heat capacity per mole of per volume |
Heat capacity
Heat capacity |
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____ will be in units of energy per degree temperature
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Heat capacity
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____ will be in energy per gram or kilogram degree Celsius molar heat or volume heat will replace the weight with moles or ml's
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Specific heat
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The ____ of water is 1 calorie per gram per degree Celsius.
For ice and steam the ____ is approx 1/2 calories per gram per degree Celsius. |
Specific heat
Specific heat |
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____ - measures heat flow at constant pressure
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Coffee cup calorimeter
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At constant pressure Q = ΔH, ____
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enthalpy change
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____ - burn or combust something in a rigid container and measure temp change in the water surrounding the container
The temperature change times the heat capacity of the calorimeter is approximately equal to the ____ of the reaction Because internal energy change only approximates ____ |
Bomb calorimeter
heat enthalpy change |
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____ - temp on the y axis and heat on the x axis
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Heat curve
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Heat curve
For the first rising segment ____, where c is the specific heat of the solid |
Q= mcΔT
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Heat curve
Second line is a flat one where temp does not change, have to use ____, simply have to multiply this by the appropriate amount of substance to find Q Sometimes the ____ is called the ____ and is represented by a L. |
enthalpy of fusion
enthalpy of fusion latent heat of fusion |
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Heat curve
The third segment is a positive slope line this starts once all the solid has melted, this line extends from the melting point to the boiling point, along this line the substance is a liquid, as energy is added the speed of the molecules in the liquid increase, as the speed increases the temperature increases Again we use the formula ____ |
Q= mcΔT
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Heat curve
The fourth segment is another flat line beginning at the boiling point. This line represents vaporization. As energy is added the bonds of the liquid are broken creating a gas. The heat of ____ is usually greater than the heat of fusion, because to ____ a substance the intermolecular forces must be completely overcome. |
vaporization
vaporize |
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Heat of fusion
The fifth segment is a positive slope line going up from the boiling point. This line represents the substance as a gas, as energy is added the speed of the molecules ____ and temperature ____. |
increases
increases |
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Heat of ____ - solid to gas
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sublimation
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Heat of ____ - solid to another solid
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transition
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Heat curve
Along the second line - increase in ____, broken bonds more movement, but decrease in ____ - energy is absorbed to break the bonds. |
entropy
enthalpy |
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____ we see that ΔG may be positive or negative, it could be spontaneous or nonspontaneous
The direction of the rxn depends upon the ____, as we would expect from a phase change. |
ΔG = ΔH - TΔs
temperature |
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___ compares - pressure on the y-axis to temperature on the x-axis
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Phase diagram
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Three area diagram - ____
____ - is up and to the left , because solids exist at high pressure and low temperature ____ - is to the right of the solid - because as temps increase solids melt ____ - lies all along the bottom of the diagram and to the right - because gases exist at low pressures and high temps |
Phase diagram
solid liquid gas |
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Ice melts under ____
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pressure
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Gas to liquid -
Liquid to gas - Solid to gas - Gas to solid - Solid to liquid - Liquid to solid - |
condensation
vaporization sublimation deposition melting freezing |
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phase diagrams
The lines represent temp and pressure values where the phases exist in ____ |
equilibrium
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phase diagram
____ - where all three lines meet, all three phases exist in equilibrium only at this point. |
Triple point
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phase diagram
____ - end of the gas/liquid line, it is determined by the critical temp and critical pressure, above the ____ gas and liquid cannot be distinguished from one another, they have the same density The substance above this point is called a ____. |
Critical point
Critical point supercritical fluid |
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____ - depend on number not kind
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Colligative properties
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The property depends not on what type but how many you have.
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Colligative properties
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4 important colligative properties -
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VFBO
Vapor pressure - more nonvolatile solute you add to the solution the lower the vapor pressure Boiling point - nonvolatile solute raises the boiling point (because of lowered vapor pressure) Freezing point Osmotic pressure |
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Boiling occurs when the vapor pressure equals the atmospheric pressure
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ΔT = KMI
K is the boiling point elevation constant of the volatile solvent M is the molality of the solution I is the vant hoff factor (the number of pieces each solute will break into when placed into solution, NaCl will break into 2 pieces for every mole added in water so theoretical vant hoff is 2, glucose dissolves but does not break down so theoretical would be 1) |
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Freezing - stuff freezes when it forms symmetrical structures, impurities inhibit symmetrical structures from forming, so adding solute to a liquid lowers the freezing point
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ΔT = KMI
Only k is the freezing point constant |
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Adding A to pure B will lower the ____
Adding B to pure A will lower the ____ There is some ratio of A to B that has the ____, as a mixture |
FP of B
FP of A lowest freezing point |
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____ - is created by solute in solution, can think of it as pulling inward while hydrostatic pressure pushed outward (good enough for the mcat)
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Osmotic pressure
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Osmotic pressure
Can also think of it as the solute molecules in solution creating their own pressure so formula: |
∏ = ImRT
I is the vant hoff factor Other factors from pv = nrt, only M is molarity |
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Utube w/ the selectively permeable membrane - solvent can move not solute
The difference between the fluid pressures on both sides is the ____ The total pressure on the side w/ the solute is just the ____. |
osmotic pressure
fluid pressure |
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osmotic pressure
Or can look at it as ____ - pure water is 0, when solute is added to water the potential drops to be negative, like most things water potential flows from high ____ to lower ____ |
osmotic potential
osmotic potential osmotic potential |