Chapter 11a Gas Laws I Chapter 11a Gas Laws I

According to the kinetic molecular theory, the kinetic energy of a gas depends on temperature and pressure

The kinetic-molecular theory states that gas particles are very far apart. What properties of a gas does this idea explain? the fluidity and compressibility

True or false True or false According to the kinetic-molecular theory, particles of a gas collide? According to the kinetic-molecular theory, particles gain and lose energy after an elastic collision? According to the kinetic-molecular theory, particles of a gas attract each other? According to the kinetic-molecular theory, particles of a gas repel each other? According to the kinetic-molecular theory, particles of a gas collide? According to the kinetic-molecular theory, particles gain and lose energy after an elastic collision? According to the kinetic-molecular theory, particles of a gas attract each other? According to the kinetic-molecular theory, particles of a gas repel each other? Gas particles neither attract nor repel each other, but they do collide in a elastic collision. Elastic Collisions result in NO net loss of energy. True False

Which substance has the lowest density, liquid water, gases water, or solid water? H 2 O(g)

A pressure of 700. kPa is equal to _____ mm Hg kPa * __1 atm_ * 760 mmHg = 101.3kPa 1 atm 5250.

The average atmospheric pressure in Denver is atm. What is this pressure in kPa? 0.830atm * 101.3kPa = 84.1atm 1 atm

If the temperature remains constant, V1V1 and P1 P1 represent the original volume and pressure, and V2 V2 P2 P2 represent the new volume and pressure, what is the mathematical expression for Boyle’s law? P 1 V 1 = P 2 V 2

Knowing the mass and volume of a gas at STP allows one to calculate the molar mass of the gas

molar volume of any gas at standard temperature and pressure (STP) 22.4L/mol

The principle that under similar pressures and temperatures, equal volumes of gases contain the same number of molecules is attributed to Avogadro

Gay-Lussac recognized that the pressure of a fixed mass of gas at constant volume is directly proportional to the Kelvin temperature. Mathematically, Gay-Lussac’s law is expressed as P = k T P = k T

Who developed the concept that the total pressure of a mixture of gases is the sum of their partial pressures? Dalton

What happens to temperature during the compression of a gas? In terms of pressure describe why? pressure and temperature are directly proportional. The temperature rapidly increases

The values for the standard temperature and pressure (STP) are P = 1 atmosphere, 760 torr T = 0°C, 273 Kelvins

Convert a pressure of 1.75 atm to kPa and to mm Hg. Convert a pressure of 570. torr to atmospheres and to kPa. Convert a pressure of 550 mm of Hg into atm and Pa Convert a pressure of 150. KPa to mm of Hg and atm

Convert each of the following Celsius temperatures to Kelvin temperatures 0.°C 27°C -75.°C -310°C.

Know how to solve gas law problems using the combined gas law. & Partial Pressure

Chapter 11b Ideal Gas Laws Chapter 11b Ideal Gas Laws

When pressure, volume, and temperature are known, the ideal gas law can be used to calculate molar amount

Calculate the approximate volume of a mol sample of gas at 15.0°C and a pressure of 1.10 atm V = nRT P 0.600mol * (15.0°C +273) = 12.9 L 1.10 atm

True or false True or false John Dalton developed the concept that the total pressure of a mixture of gases is the sum of their partial pressures? John Dalton developed the concept that the total pressure of a mixture of gases is the sum of their partial pressures? True

Who developed the Law that states that equal volumes of gas at the same pressure and temp. contain equal numbers of moles? Avogadro

If a gas with an odor is released in a room, it quickly can be detected across the room because it diffuses

True or false True or false The law of combining volumes applies only to gas volumes measured at constant temperature and pressure. The law of combining volumes applies only to gas volumes measured at constant temperature and pressure. True

The odor of perfume spreading throughout a room is an example of gas diffusion

A 1.00 L sample of a gas has a mass of 1.92 g at STP. What is the molar mass of the gas? molar mass = grams * RT PV 1.92g * * (273K) = 43.0g/mol 1.00 atm * 1.00 L

If two gases are both measured at 725 ˚C and 5.05 atm, what volume of N 2 (g) can be produced from the decomposition of 37.6 L of NH 3 (g)? 37.6 L Avogadro’s law: equal volumes of gas contain equal numbers of moles at the same pressure and temp.

Knowing the mass and volume of a gas at STP allows one to calculate the molar mass of the gas

The principle that under similar pressures and temperatures, equal volumes of gases contain the same number of molecules is attributed to Avogadro

Problem solving problem will come directly from the practice sheet If you know it you will do just fine!!!

The End!