AP Chemistry Gases Flashcards

7626903443	Gases in terms of density	Low density because the few particles are spread out in a large volume	0
7626908244	Gases in terms of compressibility	Easy to compress because the particles are spread out in a lot of empty space	1
7626910467	Gases in terms of Fluidity	Very Fluid because particles are in constant motion and aren't attracted to each other so they can move easily around each other	2
7626910468	Gases in terms of diffusion	Diffuse easily because particles are in constant motion, so they can mix freely with other types of gases. Two or more gases from a homogeneous mixture regardless of reactivity or identity	3
7626914016	Gases in terms of Effusion	Easily effuse through tiny openings because they have no shape or permanent volume.	4
7626914940	Kinetic Molecular Theory	1. Gases consist of large numbers of molecules that are in continuous random motion 2. The combined volume of all the molecules of the gas is negligible relative to the total volume in which the gas contained 3. Attractive and repulsive forces between gas molecules are insignificant 4. Energy can be transferred between molecules during collisions that are perfectly elastic but as long as the temperature stays constant, the average kinetic energy of the molecules don't change with time 5. The average kinetic energy of the molecules is proportional to the absolute temperature 6. Gases consist of tiny particles in empty space	5
7626917745	Ideal Gas	ideal gases are always gases regardless of temperature or pressure ideal gases cannot be liquified or solidified no attractive forces exist between the particles (atoms or molecules) the particles have no volume real gases behave "ideally" when the right conditions exist more ideal conditions: high temperature, high volume, low pressure, low moles	6
7626917746	Real Gas	Have volume Have attractive forces between the particles Behave ideally when high temperatures and low pressures Can be liquified or solidified	7
7626919621	Pressure	Pressure is a force exerted by the substance per unit area on another substance. P=F/A	8
7626919622	Barometer	an instrument measuring atmospheric pressure, used especially in forecasting the weather and determining altitude.	9
7626920930	Manometer	an instrument for measuring the pressure acting on a column of fluid, especially one with a U-shaped tube of liquid in which a difference in the pressures acting in the two arms of the tube causes the liquid to reach different heights in the two arms.	10
7627134407	How do you find pressure of a gas in a manometer?	P(gas)= p(atm)+p(height) in mmHg	11
7626921080	atm to mmHg	multiply by 760	12
7626923745	mmHg to Pa	multiply by 1.01325e5/760	13
7626923746	atm to Pa	multiply by 1.01325e5	14
7626923747	atm to kPa	multiply by 101.325	15
7626927462	mmHg to kPa	multiply by 101.325/760	16
7626929215	Celsius to Kelvin	Add 273	17
7626931396	Kelvin to Celsius	Subtract 273	18
7626933264	Boyle's law	The volume of a fixed quantity of gas maintained at a constant pressure is inversely proportional to the pressure. P1V1=P2V2.	19
7626936473	Charles's Law	The volume of a fixed amount of gas maintained at a constant pressure is directly proportional to its absolute value. V1/T1=V2/T2	20
7626936474	Gay Lussac's Law	The pressure of a gas is directly proportional to its Kelvin temperature. P1/T1=P2/T2	21
7626940430	Avogadro's Law	Equal volumes of gases at the same temperature and pressure contain equal numbers of moles. V1/n1=V2/n2	22
7626942586	Combined Gas Law	P1V1/T1=P2V2/T2 comes from ideal gas law	23
7626944267	Ideal gas law	PV=nRT Assumes that the molecules don't interact and the combined volume of the molecules id much smaller than the one the gas occupies	24
7626946057	R	Universal Gas Constant	25
7626946058	R in atm	0.08206	26
7626946238	R in mmHg	62.4	27
7626949547	R in kPa and Pa	8.31447	28
7626951386	Graham's Law	The rate of effusion of a gas is inversely proportional to the square root of its mass. r1/r2= the square root of MM2/MM1	29
7626953483	Absolute Zero	The temperature where all motion stops	30
7626955473	Dalton's Law	The total pressure of a mixture of gases equals the sum of the pressures that each would exert if it were present alone. P(total)=P1+P2+P3...	31
7627382313	Partial Pressure	the hypothetical pressure of that gas if it alone occupied the volume of the mixture at the same temperature.	32
7626957632	Conditions of STP	Pressure= 1atm Temperature= 273 or 0C Volume occupied by 1 mole at STP= 22.4 (molar volume)	33
7626964305	Kinetic Energy	Kinetic energy is the energy an object possesses due to its motion. KE=1/2mv^2 or KE=3/2RT	34
7626964306	Root Mean Square Velocity	v= the square root of 3(R)(T)/MM in kg/mol	35
7626967630	Conditions for most ideal gases	High Temperature Low Pressure Low moles	36
7626970352	Van der Waals Equation	mathematically deals with the non-ideality of real gases. (P + n^2a/V^2)(V-nb) =nRT	37