Chemistry, 25.10.2019 18:43 chrisraptorofficial
The vapor pressures of so2(s) and so2(l) in the vicinity of the triple point are given by the equations, ln (p/torr) = 23.9812 - 4244.7/t and ln (p/torr) = 19.2453 - 3298.4/t, respectively, where t is absolute temperature. (i)determine from these equations the three phase change enthalpies, ∆subh°, ∆vaph° and ∆fush°. (ii)show your determination of the temperature and pressure at the triple point of sulfur dioxide. (iii)assume that the enthalpy of vaporization remains at the value determined here, and show your work to predict the standard boiling point temperature of so2.
Answers: 2
Chemistry, 22.06.2019 13:50
Abeaker with 2.00×102 ml of an acetic acid buffer with a ph of 5.000 is sitting on a benchtop. the total molarity of acid and conjugate base in this buffer is 0.100 m. a student adds 4.70 ml of a 0.360 m hcl solution to the beaker. how much will the ph change? the pka of acetic acid is 4.740.
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Mercury turns to a vapor at 629.88 k. how much heat is lost when 75.0 g of mercury vapor at 650 k condenses to a liquid at 297 k?
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The vapor pressures of so2(s) and so2(l) in the vicinity of the triple point are given by the equati...
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