CHEM 1125Q 1st Edition Lecture 7 Outline of Last Lecture (Ch. 11)I. Ideal Gas Equation Flaws, Van der Waals Equation, Dalton’s Law, and Mole FractionsOutline of Current Lecture (Ch. 12)II. Intro to Liquids and SolidsA. Intermolecular ForcesIII. LiquidsA. Surface TensionB. ViscosityIV. Vapor PressureA. Vapor PressureB. Clausius-Clapeyron EquationCurrent LectureII. Intro to Liquids and SolidsA. Intermolecular Forcesa. Gas laws, such as the Ideal Gas Equation PV=nRT, can also apply to thevapors of solids and liquidsb. Liquids and solids both has strong intermolecular forces, which are the forces between formula unitsc. Intermolecular forces increase from gas to liquid to solidIII. LiquidsA. Surface Tensiona. Surface tension refers to the amount of energy required to increase orstretch the surface of a liquid b. The stronger a liquid’s intermolecular forces, the higher its surface tensionc. Liquids maximize their surface aread. Surface tension also affects capillary action, which is the movement ofa liquid up a tube. It causes cohesion and adhesioni. Cohesion is an attraction between like moleculesii. Adhesion is an attraction between unlike moleculesB. Viscositya. Viscosity is a fluid’s resistance to flowb. Higher viscosity results in slower movementThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.c. Greater intermolecular forces lead to higher viscosityIV. Vapor PressureA. Vapor Pressurea. Vapor pressure is the pressure a vapor exerts on its condensed phasesat equilibriumb. Vapor pressure is dependent on intermolecular forcesc. If the molecules at the surface have enough kinetic energy, they can escape the liquid form into gas form, a process known as vaporizationd. Vapor pressure increases until the rate of evaporation equals that of condensation, or equilibriume. Dynamic equilibrium is when the forward and backwards processes ofa chemical equation have the same ratef. There is a limited amount of heat that can be applied in order to raise the pressureg. Vapor pressure always rises with temperaturei. The temperature at which Pvapor = 1 atm is a vapor’s normal boiling pointh. Solving for vapor pressure requires the use of natural logs and exponentsi. The natural log (ln) is based on the value eii. e = 2.71828…iii. Algebra with logs:ln(ex) = xln(x)y = yln(x)ln(x/y) = ln(x) – ln(y)ln(xy) = ln(x) + ln(y)B. Clausius-Clapeyron Equationa. The Clausius-Clapeyron Equation relates the natural log of vapor pressure to the reciprocal of absolute temperaturei. lnP = - ΔHvapor/RT + Cb. The Clausius-Clapeyron Equation can also be written as:i. Ln(P1/P2) = (ΔHvapor/R)(1/T2 – 1/T1)Here the R value is 8.3 J/mol Kc. The boiling point is equivalent to the temperature at which vapor pressure equals the external atmospheric pressured. The boiling point varies with the external pressure and the magnitudeof intermolecular forcese. Normal boiling point is the temperature when the vapor pressure equals 1