In Exercise 112 in Chapter 5, the pressure of CO2 in a bottle of sparkling wine was calculated assuming that the CO2 was insoluble in water. This was an incorrect assumption. Redo this problem by assuming that CO2 obeys Henry’s law. Use the data given in that problem to calculate the partial pressure of CO2 in the gas phase and the solubility of CO2 in the wine at 25oC. The Henry’s law constant for CO2 is 32 L atm/ mol at 25oC with Henry’s law in the form P = kC, where C is the concentration of the gas in mol/ L.
Answer to relevant QuestionsRationalize the temperature dependence of the solubility of a gas in terms of the kinetic molecular theory. The freezing point of t-butanol is 25.50oC and Kf is 9.1oC kg/mol. Usually t-butanol absorbs water on exposure to air. If the freezing point of a 10.0-g sample of t-butanol is 24.59oC, how many grams of water are present in ...In the winter of 1994, record low temperatures were registered throughout the United States. For example, in Champaign, Illinois, a record low of 229oF was registered. At this temperature can salting icy roads with CaCl2 be ...Hydrogen is produced commercially by the reaction of methane with steam: CH4(g) + H2O(g) ⇌ CO(g) + 3H2(g) a. Calculate ΔHo and ΔSo for this reaction (use the data in Appendix 4). b. What temperatures will favor product ...Write equations describing the reactions of Ga with each of the following: F2, O2, S8, and HCl.
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