GAS LAWS FLIPBOOK

GAS LAWS FLIPBOOK By: Natalia Pastor-Navarro 4B HHS

Table of Contents Kinetic Molecular Theory Volume Temperature Pressure Ideal Gasses Law Avoradgo Principle/ Molar Volume Boyles Law Charles Law Gay-Luccas Law Combined Gas Law Practice Problems

Kinetic Molecular Theory ❖ General Properties of Gasses ➢ The Quantity of Gas, n (in moles) ➢ The temperature of the gas, T (in Kelvins) ➢ The volume of gas, V (in liters) ➢ The pressure of the gas, P(in the atmosphere) ❖ What is the Kinetic Molecular Theory? ➢ An explanation of the kinetic motion in our atmosphere ➢ Now there are a couple of assumptions of the Model which includes ■ All particles are in constant, random, motion ■ All collisions between particles are perfectly elastic, which means that there is an even exchange of energy ■ The volume of the particles in a gas is negligible ■ The average kinetic energy of the molecules is its Kelvin temperature ➢ However, it is important to note that this theory does not assume that there are any intermolecular forces. ➢ It is also necessary to note that unlike solids/liquids gases to expand to fill its container and are all compressible

Pressure ❖ Definition- Refers to the number of collisions that gas particles have with their containers or surroundings. Or the measure of force a gas exerts on its container ❖ Units ➢ Force/ unit area; N/m^2; which is the definition of 1.0 Pascal ➢ The SI unit of pressure is the Pascal (after Blaise Pascal); 1 Pa = 1 N/m^2 ❖ How do we measure this ➢ The barometer: invented by Evangelista and used the height of a column of mercury to measure gas of pressure ➢ Often uses 1.00 atm, 760 mm Hg, 101.325 kPa ➢ Manometer: a device for measuring the pressure of a gas in a container ➢ The pressure of the gas is given by h (the differences in mercury levels) in units of torr (equivalent to mm Hg) ➢ Gas pressure = atmospheric pressure-h; you do this Gas pressure (P) less than atmospheric pressure ➢ Gas pressure = atmospheric + h; you do this when Gas pressure (P) greater than atmospheric pressure

❖ Conversion methods ➢ To convert 760 mmHg = 1 atm = 101.3 kPa = 760 torr= 29.92 Hg= 4. psi= 10^5 Pa ➢ Use dimensional analysis ➢ EX: 49 torr| 1 atm| = 0.064 atm | 101.3 KPa | 10^3 Pa = 760 torr 1 atm 1 KPa

Volume ❖ Definition- Volume is the amount of space occupied by a substance, while mass is the amount of matter it contains. The amount of mass per unit of volume is a sample's density. ❖ Units- We measure the volume in Liters and it is known as V ❖ How do we measure the volume? We typically use a beaker or graduated cylinders to measure. There is sometimes when using displacement for an irregular shape. ❖ Conversions methods- 1 L is equivalent to 1,000 ml. We can use dimensional analysis to get the volume. In addition, 1 g is equal to 1 ml.

Temperature ❖ Definition- Temperature itself is the measurement of the average kinetic energy of a substance. ❖ Units- We measure the temperature also known as T in Kelvin. ❖ Conversions methods- 273 Kelvin is equal to 0 Celcius. 0 celsius is equal to 32 F. We can use dimensional analysis to get the temperature.

Ideal Gasses Law ❖ Ideal Gases are gases that exist only in ideal conditions because they limit attractive forces ❖ What we want an Ideal Gas to be ➢ They Obey KMT at all times ➢ Do not take up any space (no volume) ➢ Have no effect on each other (no IMF attractions or repulsions) ➢ Obey the ideal gas laws under all conditions ➢ However, it is important to note that in the real world no gas is truly ideal ❖ i. Statement of the law- a description of gas behavior that permits you to solve for the number of moles of a contained gas when given only ONE VALUE EACH for P, V, and T. ❖ Which variables are related ❖ Which variables are constant- the Ideal Gas Constant is R, 0.0821 is L * atm/ mol * k, 62.4 L* mmHg ❖Formula: PV = nRT

➢ Important to note everything must be in the same units

Avoradgo Principle/ Molar Volume ❖ Statement of the principle- If pressure and temperature are held constant, then the volume of gas directly proportional to # of moles of gas present ❖ Conversion factors (design a map) ❖ Volume and number of moles ❖ Constant- pressure and temperature ❖ STP- a standard temperature which is 0 degrees Celsius or 273 degrees Calvin. In addition, it must be at the standard pressure of 101.3 kPa (1 atm) ❖ Molar Volume- this is the volume that one mole of gas occupies at STP. It is 22. 4 L ❖

Boyles Law ❖ Statement of the law- The volume of a confined gas is inverley proportional to the pressure exerted on the gas ➢ Volume and Pressure are at a constant temperature ❖ Which variables are related- Volume and Pressure ❖ Which variables are constant- Temperature ❖ Formula- P1 V1 = P2 V2 Boyle’s law ❖ Graphic representation of the relationship ❖ However it is important to note that this Law only applies when it is at low pressures

Charles Law ❖ Statement of the law- If a given quantity of gas is held at a constant pressure, then its volume is directly proportional to the absolute temperature (we must use Kelvins, which masures average kinetic energy) ❖ Who made this law- Jacques Charles was a French physicist who filled a hot air balloon with hydrogen gas and made the first solo hot air balloon flight! ❖ Formula- V1 T2 = V2 T1 or V1 / T1 = V2 / T2 ❖ Which variables are constant- Pressure ❖ Which variables are related- Temperature and Volume (directly related) ❖ Graphic representation of relationship-

Note about graph- The samples of the various gases contain different number of moles Absolute zero (theortical volume)

Gay-Luccas Law ❖ Statement of the law- Volume of gases always combine with one another in the ratio of small whole numbers, as long as volume ar measured at the same T and P ➢ If the temperature increases the temperature also increases (directly proportional) ❖ Formula- P1 T2 = P2 T1 or P1/ Ti = P2/ T2 ❖ Which variables are constant- Volume ❖ Which variables are related- Temperature and Pressure(directly related) but only if the container is not expandable ❖ Graphic representation of relationship- ❖

Avogrados Law ❖ Statement of the law- The volume of a gas, at a given temperature and pressure, is directly proprotional to the quantity of gas you havee ❖ If the temperature increases the temperature also increases (directly proportional) ❖ Formula- V1 / N1 = V2/ N2 ❖ Which variables are constant- Temperature and Pressure ❖ Which variables are related- Volume and moles ❖ His hypothesis- Equal volumes of gases under the same conditions and pressure contain equal numbers of molecules ❖ Graphic representation of relationship- ❖ Important note- These balloons each hold 1.0 L of gas at 25 C and 1 atm. Each balloon contain 0.041 mol of gas or 2.5 x 10 ^22 gas molecules

Combined Gas Law ❖ Statement of the law- Combined the Laws of Boyle, Charles and Gay-Lussac ❖ Which variables are related- Volume Temperature Pressure (don’t know which one is having to affect) ❖ Which variables are constant- Moles ❖ Formula- P1 V1 N1 T1 = P2 V2 /N2 T2 or P1 V1/ Ti = P2 V2 = T2N2 (alot of times leave N out of equation)

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Practice Problems