the physical properties of gases
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| A FORCE APPLIED OVER A UNIT AREA | PRESSURE
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| INCREASES WHEN THE APPLIED FORCE INCREASES OR THE AREA OVER WHICH IT IS APPLIED DECREASES | PRESSURE
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| FORCE/AREA | =PRESSURE
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| 1 MOL OF GAS = | 22.4 L
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| THE WEIGHT OF THE ATMOSPHERE PRESSING AGAINST THE EARTH'S SURFACE | ATMOSPHERE PRESSURE
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| ATMOSPHERE PRESSURE IS MEASURED BY AN INSTRUMENT CALLED | BAROMETER
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| 1 ATM= | 760 TORR = 76O MM HG
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| THE ACTUAL FORCE OF THE ATMOSPHERE PUSHING ON A SURFACE ARISES FROM INDIVIDUAL RAPIDLY MOVING GAS MOLECULES IN THE ATMOSPHERE BOUNCING OFF THE SURFACE | ATMOSPHERIC PRESSURE
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| PRESSURE | P
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| VOLUME | V
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| NUMBER OF MOLES | n
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| KELVIN TEMPERATURE | T
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| INCREASING THE PRESSURE WILL DECREASE THE VOLUME. NUMBER OF MOLES & TEMPERATURE HELD CONSTANT.(INVERSELY PROPORTIONAL) | BOYLE'S LAW
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| BOYLE'S LAW | P1*V1=P2*V2
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| INCREASING THE TEMPERATURE WILL INCREASE THE VOLUME.WHEN PRESSURE & NUMBER OF MOLES OF GAS ARE HELD CONSTANT. (DIRECTLY PROPORTIONAL) | CHARLES'S LAW
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| CHARLES'S LAW | V1/T1=V2/T2
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| GAY-LUSSAC'S LAW | P1/T1=P2/T2
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| PRESSURE & TEMPERATURE OF A GAS WHEN THE VOLUME & NUMBER OF MOLES ARE HELD CONSTANT | GAY-LUSSAC'S LAW
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| VOLUME OF A GAS TO THE NUMBER OF MOLES OF GAS PRESENT WHEN THE PRESSURE AND TEMPERATURE ARE HELD CONSTANT | AVOGADRO'S LAW
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| AVOGADRO'S LAW | V1/n1=V2/n2
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| COMBINED GAS LAW | P1*V1/T1=P2*V2/T2
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| HELPS US CALCULATE THE NEW VALUE OF ONE OF THE VARIABLES WHEN BOTH OF THE OTHERS ARE CHARGED SIMULTANEOUSLY | THE COMBINED GAS LAW
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| THE IDEAL GAS LAW | PV=nRT
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| PV/nT | CONSTANT
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| UNIVERSAL GAS CONSTANT | R
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| ALL 4 VARIABLES, P,V,n,T, CAN BE COMBINED INTO THE FOLLOWING SINGLE MATHEMATICAL EXPRESSIONS CALLED | IDEAL GAS LAW
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| WHEN 2 DIFFERENT GASES ARE MIXED TOGETHER, THEIR BEHAVIOR IS DESCRIBED BY | DALTON'S LAW OF PARTIAL PRESSURES
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| DALTON'S LAW OF PARTIAL PRESSURES | P(total)=P(A)+P(B)
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| The gas consists of very small particles, all with some mass. | Ideal Gas
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| The number of molecules is large such that statistical treatment can be applied. | Ideal Gas
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| These molecules are in constant, random motion. The rapidly moving particles constantly collide with the walls of the container. | Ideal Gas
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| The collisions of gas particles with the walls of the container holding them are perfectly elastic. | Ideal Gas
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| The interactions among molecules are negligible. They exert no forces on one another except during collisions. | Ideal Gas
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| The total volume of the individual gas molecules added up is the negligible compared to the volume of the container. The molecules are perfectly spherical in shape, and elastic in nature. | Ideal Gas
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| The average kinetic energy of the gas particles depends only on the temperature of the system. | Ideal Gas
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| P(atmosphere)=P(gas)+P(water) | Dalton's Law of Partial Pressures
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| General Rule: the greater gas's partial pressure in a gas mixture, the greater the extent to which that gas will dissolve in any liquid present. | Henry's Law
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| (amount of gas dissolved/Unit volume of solvent)=C(h)* gas pressure | Henry's Law for a Pure Gas
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| (Amount of gas dissolved/Unit volume of solvent)= C(h)* gas partial pressure | Henry's Law for a Mixture of Gases
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| C(h) | Henry's Law Constant
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| (amount of gas dissolved/within a unit volume of solvent)/ gas pressure | =C(h)
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| C(h)= | mL gas/mL solvent * atm
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| gas decreases as the temperature increases | solubility
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| pressure (P), volume (V), temperature (T), Number of Moles (n) | properties of gases
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| The amount of a gas that will dissolve in a liquid depends chiefly on the gas pressure & is described by Henry's law. As the gas pressure increases, more gas will dissolve. | Gases in Liquids
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| Solid, liquid, gas | 3 stages of matter
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| fixed volume, fixed shape | solid
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| fixed volume, no fixed shape | liquid
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| no fixed volume, no fixed shape | gas
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| volumes change very little when pressure is applied | solids/liquids
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| constituent molecules are touching but not so highly ordered | solids
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| constituent molecules are touching but not so highly ordered | liguid
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| constituent molecules are not touching and are highly disordered | gas
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| molecules move at highspeeds and change directions only when they hit the walls of their container (pressure) or each other | gas
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| do not collide often, so often, so attractive forces between molecules have little effect. | gaseous molecules
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| energy of motion | kinetic energy
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| kinetic energy is directly related to temperature | at molecular level
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| opposes the attractive forces between molecules | kinetic energy
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| a solid may melt to the corresponding liquid when heat is added | melting
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| a liquid may feeze to the corresponding solid when heat is removed | freezing
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| a liquid may boil to the corresponding gas when heat is added | vaporization
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| a gas may condense to the corresponding liquid when heat is removed | condensation
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| melting/freezing and boiling/condensation | examples of phase transitions (reversible)
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| the total amount of heat required to melt on mole of a substance and is unique for each substance | molar heat of fusion )H
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| the total amount of heat required to boil one mole of a substance and is also unique for each substance. The molar heat of vaporization is always much greater than the molar heat of fusion | molar heat of vaporization )H
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| the exchange or sharing of electrons between ATOMS and IONS | chemical bonds
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| electrons are completely transferred from one atom to another (polar) | ionic bond
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| electrons are shared between atoms-the sharing is not always equal(Polar-equal, non polar-non equal) | covalent
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| between | inter
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| within | intra
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| these forces are those responsible for holding solids and fluids together | intermolecular forces
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| these forces are responsible for the correct folding of protein and other large biomolecules | intramolecular forces
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