CHEM 135 1st Edition Lecture 7Outline of Last Lecture I. Review of freezing point depression and boiling point elevationa. ExamplesII. OsmosisIII. Osmotic PressureOutline of Current Lecture I. Questions from Chapter 12 worksheet + answersII. Beginning of Chapter 13-Chemical KineticsCurrent LectureChapter 12: Solutions (worksheet)1. The Henry’s Law constant of methyl bromide is k=0.159 mol/(L*atm) at 25°C. What isthe solubility of methyl bromide in water at 25°C and at partial pressure of 270 mm Hg?a. 0.0565 mol/Lb. 0.355 mol/Lc. 0.448 mol/Ld. 42.9 mol/L2. A solution is prepared by dissolving 40.0 g of sucrose in 250 g of water at 25°C. What is the vapor pressure of water at 25°C is 23.76 mm Hg?a. 0.198 mm Hgb. 20.5 mm Hgc. 23.6 mm Hgd. 24.0 mm Hg3. Determine the boiling point of a solution that contains 78.8 g of naphthalene dissolved in 722 mL of benzene. Pure benzene has a boiling point of 80.1°C and a boiling point elevation constant of 2.53°C/m. a. 2.2°Cb. 2.5°Cc. 80.4°CThese 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.d. 82.6°C4. Calculate the osmotic pressure of the solution containing 1.5 g of ethylene glycol in 50 mL of solution at 25°C.a. 8.5 atmb. 11.8 atmc. 12.4 atmd. 24.0 atmChapter 13: Chemical KineticsRate of a chemical reaction:- Rate= ∆ concentration∆ time- Speed= mileshourRate-change in concentration of a reactant or product as a function of time∆= final*initialA (reactant consumed) >> B (product formed), rate=−∆ ( A)T- It is negative because the rate is decreasingLaw of conservation:∆( A)∆(T )=∆(B )∆
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