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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:The enthalpy of vaporization of Substance X is 18.0-
and its normal boiling point is -93. °C. Calculate the vapor pressure of X at -129. °C.
mol
Round your answer to 2 significant digits.
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- How many moles of CO2 (g) are present after 25.0 mL of dry ice sublimes? Do not include the unit of measure in your answer.arrow_forwardDiethyl ether (molar mass 74.12 g/mol) boils at 34.6 °C and water (molar mass 18.02 g/mol) boils at 100 C. a. At 25 °C, which compound – diethyl ether or water – has the higher vapor pressure? b. Which data – molar mass or boiling point – did you use to make your choice? Explain your answer.arrow_forwardA sample of C3H4Br2 has a normal boiling temperature of 131.5 °C. The enthalpy of vaporization for this compound is 35.4 kJ/mol. What would be the boiling temperature in °C of C3H4Br2 at a pressure of 540.0 mm Hg? Report your answer using three significant figures.arrow_forward
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