Gas Behavior

Master ideal gas behavior! Learn real vs. ideal gases, STP, and Avogadro's Law with practice problems.

Part 1: What is an Ideal Gas? Use the following text to sort the statements.All gases are real, but what makes them Ideal?Real gases have mass and volume. After all, they are made of atoms and molecules like all matter. They bounce off each other and the container in which they are being held. The force of the bounce is what we measure as the pressure inside the container. Just like all things that bounce, real gas molecules lose some of their energy to the sides of the container they hit, and even to other molecules when they collide. Volume is determined by the size of the container, and temperature is the average kinetic energy of the particles in the container.Ideal gases follow the Ideal Gas Law. That means, that in an ideal gas, it does not matter how closely packed in the molecules of the gas are, they do not interact with each other (don't become a liquid or solid). It also means that they do not lose energy when they collide with each other or the container, and they basically have no volume, their molecules are just points with no density.Do any gases actually act like these "Ideal" gases? You probably said "No!" and you are correct. So why do we have to learn this? As a gas becomes less dense, either hotter, lower pressure, and increased volume, the more it acts like an "Ideal" gas. So, if we know pressure, temperature, and volume, we can use the Ideal Gas Law to do stoichiometry problems involving gases and obtain very realistic answers.[retrieved from Real Gas Has mass and volume Is a liquid at high pressure Particles lose energy with each collision Ideal Gas Stays gaseous at low temperature Has elastic collisions Has no volume Part 2: What is STP?✔ STP stands for Standard Temperature and Pressure. It is defined as 273K at 1 atmosphere pressure.✔ All temperatures used in problems with gasses must use the Kelvin (absolute) temperature scale.To convert from degrees C to degrees Kelvin, remember "K is C plus 273" (degrees C + 273 = K)✔ 1 atmosphere of pressure can also be expressed as 101.3 Kilopascals, or 760mmHg (millimeters of mercury).This information gives us the conversion fractions:1 atmOR1 atmOR760 mmHg101.3 Kilopascals760 mmHg101.3 KilopascalsTASK: Convert 35oC to Kelvin 238K 308K 273K 173K Task: Convert 395K to degrees Celsius 668oC 100oC 135oC 122oC STP is 273K and 4 atm 3 atm 2 atm 1 atm Task: Convert -25oC to Kelvin 298K 273K -273K 248K Task: Convert 2.3 atm to mmHg 1,748 mmHg 275 mmHg 330 mmHg 760 mmHg STP means standard temperature and pressure standard thermometer pressure selected thermal pressure units Stand-alone Temperature and Pressurized gas Task:Convert 500 mmHg to atm 380,000 atm 0.66 atm 101.3 atm 100 atm Task: Convert 2.3 atm to kpascals 44 kpascals 101.3 kpascals 233 kpascals 0.02 kpascals Part 3 Match the Terms Match the terms with the statement, number or formula Avogadro's Constant (number) 6.02e23 Pressure atm Mass g Volume L Mole mol 22.4L the volume of 1 mole of any kind of gas 6.02e23 the number of particles in 1 mole of a substance Molar mass the number of grams (from the PT) of the element or compound in 1 mole of that substance Part 4: Avogadro's Law Avogadro's Law states that in the same volume of any gas, at the same temperature and pressure, there is the same number of molecules or atoms. Watch the video carefully and then answer the following questions. Under the same conditions of temperature and pressure, equal volumes of all gasses contain the same atomic masses proportional chemical formulas the same number of molecules. differing volumes For the diagram above, which of the following is FALSE? They contain n and 2n number of moles respectively They contain the same number of moles The volume of the container on the right is twice the volume of the container on the left The temperature and pressure for both containers is constant 22.4 L of NH3contains 22.4 L of H2 28.0 g of N2 17.0 g of NH3 2 moles of NH3 22.4 L of NH3contains 6.02e23 particles of NH3 28.0 g of N2 32.0 g of O2 2 moles of NH3 2 moles of NH3 has the same number of particles as 1 moles of O 28.0 g of N2 56.0 g of O2 2 moles of O2 Fill in the blanks using calculations from the information found in the diagram below. One mole of NH3 has a mass of 17.0 gand a volume of 22.4 Lat STP. 0.35 moles of CO2 would have a mass of 15.4 g and contain 2.11e23particles.1.5 moles of H2 contains 9.03e23molecules or particles and has a mass of 3.0 g.1 mole of SO2 contains 6.02e23molecules or particles and has a mass of 64.0 g.0.5 moles of SO4 and 0.5 moles of CO2 both contain 3.02e23molecules or particles.