Lecture 15Outline of Last LectureI. Molecular Orbital Theory (MO Theory)A. HOMO and LUMO.II. Bonding MO’sIII. Antibonding MO’s IV. Nonbonding MO’sA. Acceptable and Unacceptable MO bondingOutline of Current LectureI. Ideal Gas LawA. Boyle’s LawB. Charles’ LawC. Avogadro’s LawD. Gay-Lussac’s LawII. MolarityIII. Finding the Pressure of a Gas in a Manometer.Current LectureI. Ideal Gas Law: PV = nRT- The Ideal Gas Law is an equation that relates different characteristics of a substance based on their correlation. These correlations are between pressure (P), volume (V), temperature (T), Amount of moles (n) and the Ideal Gas Law constant 0.0821 (R). Ex) What is the pressure inside a 7.20L container filled with 13 grams of CO2 at 35o C?This equation requires some conversions before plugging in the numbers into the ideal gas law.Convert:13g CO2 -> moles CO213g CO2 * 1 mol/44.01 g CO2 = 0.295 mol CO2, n = 0.295 molConvert:35o C -> Kelvin35 + 273 = 308 K, T = 308 KPlug into PV = nRT:(P)(7.2) = (0.295)(0.0821)(308) CH 101 1st EditionP = 1.03 atmA. Boyle’s Lawo Boyle’s law states that pressure and volume are inversely related, PV = PV.B. Charles’ Lawo Charles’ law states that volume and temperature are directly proportional, V/T = V/T.C. Avogadro’s Lawo Avogadro’s law states that volume and the number of moles is directly related which is commonsense, V/n = V/n. This law also tells us that 22.4 Liters = I mole.D. Gay-Lussac’s Lawo This law states that pressure and temperature are directly related, P/T = P/T II. Molarity- Molarity can be found by using the equation Moles/Liters or n/V. Molarity and molar concentration are the same thing.III. Finding the Pressure of a Gas in a Manometer.- A manometer is a type of beaker that can hold a gas and measure the pressure. When given a picture of a manometer, if the gas has a higher pressure than the atmosphere (if the gas is pushing down the mercury more than the atmosphere) the equation is:(Pressure of the atmosphere + the change in height) = Pressure of gas (atm)If the pressure of the gas is less than the pressure of the atmosphere the equation is:(Pressure of the atmosphere - the change in height) = Pressure of gas (atm)Ex)The pressure of the gas would be found by taking 766 mm Hg + 250 mm = 784 mm HgTo convert this to atm just divide by 760 (mm Hg/atm) because 1atm = 760 mm Hg784 mm Hg / 760 (mm Hg/atm) = 1.03