mperatures. The sketches are drawn as if a sample of hydrogen chloride were under a microscope so powerful that individual atoms could be seen. Only on ketch in each set is correct. se the slider to choose the correct sketch in each set. You may need the following information: melting point of HCl: -114.8 °C boiling point of HC1: -85.1 °C A B C (Choose one) (Choose one) (Choose one)

In a mountainous location, the boiling point of pure water is found to be 95C. How many grams of sodium chloride must be added to 1 kg of water to bring the boiling point back to 100C? Assume that i = 2.

Consider two hypothetical pure substances, AB(s) and XY(s). When equal molar amounts of these substances are placed in separate 500-mL samples of water, they undergo the following reactions: AB(s)A+(aq)+B(aq)XY(s)XY(aq) a Which solution would you expect to have the lower boiling point? Why? b Would you expect the vapor pressures of the two solutions to be equal? If not, which one would you expect to have the higher vapor pressure? c Describe a procedure that would make the two solutions have the same boiling point. d If you took 250 mL of the AB(aq) solution prepared above, would it have the same boiling point as the original solution? Be sure to explain your answer. e The container of XY(aq) is left out on the bench top for several days, which allows some of the water to evaporate from the solution. How would the melting point of this solution compare to the melting point of the original solution?

Heat is released when some solutions form; heat is absorbed when other solutions form. Provide a molecular explanation for the difference between these two types of spontaneous processes.

A 0.500-g sample of KCl is added to 50.0 g of water in a calorimeter (Figure 5.12). If the temperature decreases by 1.05 °C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the specific heat of the resulting solution is 4.18 J/g °C? Is the reaction exothermic or endothermic?

ou place hot metal into a beaker of cold water. ol type='a'> Eventually what is true about the temperature of the metal compared to that of the water? Explain why this is true. i>Label this process as endothermic or exothermic if we consider the system to be the metal. Explain. the water. Explain.

If a substance has a positive enthalpy of solution, which would likely cause more of it to dissolve, hot solvent or cold solvent? Explain.

Describe, on both a microscopic and a macroscopic basis, what happens to a sample of water as it is cooled from room temperture to 50Cbelow its normal freezing point.

Convert the units of Henrys law constant for CO2, in table 7.2, to units of, mmHg, atm, and bar. In which cases does the numerical value of the constant change?

8.52 Rank the following hydrocarbons in order of increasing vapor pressure: C2H6,C10H22,CH4,C7H16,C22H46 .