Gas Laws Flipbook

Gas Laws Flipbook By: Akhil Revuru 3A

Properties of gases “ The Gaseous state of matter is the simplest and well-known states of matter” The four quantities that define gas: Quantity→ moles Temperature→ Kelvins Volume→ Liters Pressure→ how many collisions of gas molecules (atmospheres) Let’s start with the KINETIC MOLECULAR THEORY OF GASES- This is a theory that examines why Gases behave in the way that they do Assumptions of this theory: -All particles are in constant, random motion -All collisions between particles are perfectly elastic (equal exchange of energy) -The volume of the gas particles are not worth considering -The average kinetic energy would be named as the kelvin temperature

Properties of gases cont. Another important gas variable to talk about is… GAS PRESSURE - how many collisions that molecules have Increased collisions→ increased pressure ** The SI unit of pressure would be a Pascal 1Pa=1 N/m2 How to measure the pressure?- The Barometer uses mercury to measure atmospheric pressure 1 mmHg→ 1 torr The Standard Pressure would be: 1.00 atm→ 760.00 torr→ 760 mmhg→ 101.325kPa How to solve for gas pressure? Gas pressure= atmospheric pressure - h Gas pressure = atmospheric pressure + h

Ideal gas law and Molar Volume Ideal gases only happen in ideal conditions and are not real gases!!! Put in high temperature and low pressure DEAL GAS LAW: It is the description of gas behavior that can solve for different variables. PV= nR(pressure unit)T **volume is always in liters, temperature must be in Kelvin Ideal Gas constants: 0.0821 L * atm/mol * K 62.4 L * mmHg/mol * K 8.314 L * kpa/mol * K

Molar Volume Similar to molar mass, however it only works with gases. It is the volume that one mole of gas would occupy. STP Conditions (set conditions): 1 mole standard volume: 22.4 L, standard temperature: 273 K (0C), standard pressure: 101.3 kPa (1 atm) New conversion factor (only gases): 22.4L = 1 mol at STP **if pressure and temperature were held constant, the volume would be proportional to the # of moles of gases**

Experimental gas law 1. Boyle’s law- the volume of a confined gas is inversely proportional to the pressure exerted by gas at a constant temperature. This law holds true only under low pressure!!! P1V1=p2v2 ----> easiest formula of Boyle’s law 2. Charles’ Law- If the quantity of a gas in kept at a constant pressure, the volume is directly proportional to the absolute temperature at a constant pressure. Must use Kelvins!! If temperature increases the volume increases as well V1/T1 = V2/T2

Experimental gas law 3. Gay-Lussac’s law- At a constant volume, pressure and temperature of the gases are directly related. If the pressure increases and the container is not expandable, the temperature increases. P1/T2 = P2/T2 **the more the temperature the more the collisions 4. Avogadro's Law- The volume of a gas, at a certain temperature and pressure, is directly proportional to the quantity of gas. The more moles of gas the more volumes of gas increased. V1/N1 = V2/N2

Combined gas law The combined gas law is the combination of all of the experimental laws, and allows for us to calculator for more than one variable changes. P1 V1/T1 N1 = P2 V2/T2 N2

Practice Problems