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Chem Final Unit 2

This will contain important questions needed to know on unit 2

QuestionAnswer
What happens when gases behave? It is easier to describe their behavior theoretically, experimentally, and mathematically. almost never behave themselves
What are the 3 gas laws and what do they use? Boyles Law - pressure and volume, Charle's Law - volume and temperature, Avogadro's Law - volume and moles
What are the equations of Boyles Law, Charles' Law, and Avogadro's Law? Boyles Law - P1V2 = P2V2, Charles' Law - V1T1 = V2T2, Avogadro's Law - V1/n1 = V2/n2
What is the Ideal Gas Law formula of these combined laws? PV = nRT
What is special about gases? They bounce around each other creating pressure
What is special about Boyle's Law? Pressure and volume are inversely proportional
What is special about Charles' Law? Volume and temperature are directly proportional
What is the Kinetic Molecular Theory? explains the behavior of gas and contains 5 postulates deriving ideal gas laws
What is Postulate 1? particles of a gas are in constant motion and collide with one another and the container -- tiny particles like atoms are subject to laws of motion
What is Postulate 2? the gas is mostly empty space (dimensionless points)
What is Postulate 3? pressure is exerted when the particles hit the sides of the container -- collide with wall = loss of kinetic energy
What is Postulate 4? we assume that the particles don't intersect with each other -- the slight interactions are negligible dispersion integers or dipole-dipole integers if molecule. = polar purely elastic --> no loss of kinetic energy --> bounce off
What is Postulate 5? average kinetic energy is proportional to the temp of gas in K -- increase of temperature = increase of kinetic energy --> particles move faster If temperature goes up particles move faster
What is a gas? A phase of matter where atoms of substances are in motion and fill their container
What are the 2 importance parts of a gas? 1) Particles of a gas are dimensionless points in random motion 2) Particles don't come apart from elastic collisions
What does each of the parts of the Ideal Gas Law, PV = nRT, mean? P = pressure V = volume n = moles R = molar gas constant T = temperature
What is special about Avogadro's Law? equal volume of gas at the same temperature and pressure contain the same number of molecules
If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? R = 0.0821 L*atm/K*mol 204.63 K
If I have an unknown quantity of a gas at a pressure of 0.5 atm, a volume of 25 liters, and a temperature of 300K, how many moles of gas do I have? R = 0.0821 L*atm/K*mol 0.508 mol
A ballon that contains 1.50L of air at 1.00 arm is taken underwater to a depth at which the pressure is 3.00 atm. Calculate the new volume of the balloon. Assume the temperature remains constant. 4.5L
A sample of krypton gas occupies 75.0 mL at 0.400 atm. If the temperature remained constant, what volume would the krypton occupy at 4.00 atm? 0.75 L
A gas sample contained in a cylinder equipped with a movable piston occupied 300.0 mL at a pressure of 2.00 atm. What would be the final pressure if the volume were incresed to 500.0 mL at a constant temperature? 3.33 atm
Several balloons are inflated with helium to a volume of 0.75 L at 27C. One of the balloons was found several hours later, the temperature had dropped to 22C. What would be the volume of the balloon when found, if no helium has escaped? 0.74L
A sample of gas occupies a volume of 7.5L at 28.0C. At what temperature is the volume of the gas 4.00 L is the pressure is kept constant? 160.5 K
A 280.0 mL sample of neon exerts a pressure of 660.0 torr at 26.0C. At what temperature would it exert a pressure of 940.0 torr in a volume of 440. mL assuming the number of moles remains constant? T2 = 669.2K
A fixed quantity of gas at 23.0C has a volume of 10.3 L. Calculate the volume the gas will occupy if the temperature is increased to 145C while the pressure is held constant. v2 = 14.55L
A gas initially at STP is changed to 248 K. Calculate the final pressure of the gas. P2 = 0.908 atm
A sample of gas has a pressure of 700.0 mmHg and 30.0 C. At what temperature would the pressure be 600. mmHg if the volume remains constant? T2 = 259.71 K
A given sample of gas has a volume of 4.20 L and 1.00 atm pressure. Calculate its pressure if the volume is changed to 5.00 L and the temperature to 27C. P2 = 0.757 atm
What are the gas pressure unit conversions? 1 atm = 760 torr = 101.3kPa = 760 mmHG = 14.7psi
The pressure of a gas is 725 torr. What is the pressure of this gas in atm? 0.954 atm
The pressure of the air at a certain valley below sea level is 117 kPa. What will be the height of the mercury column in a barameter? 877.8 mmHg
What happens when elevation drops? Pressure increases
What is Gay Lussac's Law? P1/T1 = P2/T2
What is the constant of Gay Lussac's Law? mass and volume
What is important about Gay Lussac's Law? pressure and temperature are directly proportional
What does 1 mole of gas = in L? 22.4 L
What are the standard temperatures? 0C and 273 K
What are the standard pressures? 1 atm, 760 mmHg, and 760 torr
What volume will 1.27 moles of helium gas occupy at STP? 28.4 L
A sample of argon gas at STP occupies 56.2 L. Determine the number of moles of argon and the mass of argon in the sample. 100.3 g Ar
Given the following rxn: CuO (s) + H2 (g) --> CU (s) + H2O (g). If 250.0L of hydrogen gas is used to reduce copper (II) oxide at STP, what mass of copper is to be expected? 709.3 g Cu
Given the following rxn: Li (s) + 2H2O (l) --> H2 (g) + 2 LiOH (aq). How many grams of solid lithium must be added to liquid water to obtai 15.0 L of hydrogen gas at STP? 4.65 Li
Created by: pandabear66*
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