Part A Vapor pressure data (in atm) for water as a function of temperature (K) are collected. A linear regression fit of a plot of In P vs. 1/T yields a straight line described by the equation: y = -4696.9x + 18.97 Determine the enthalpy of vaporization of water in kJ/mol. R = 8.314 J/mol K Report your answer to 2 decimal places. ▾ View Available Hint(s)

Part A Vapor pressure data (in atm) for water as a function of temperature (K) are collected. A linear regression fit of a plot of In P vs. 1/T yields a straight line described by the equation: y = -4696.9x + 18.97 Determine the enthalpy of vaporization of water in kJ/mol. R = 8.314 J/mol K Report your answer to 2 decimal places. ▾ View Available Hint(s)

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter14: Liquids And Solids

Section: Chapter Questions

Problem 4QAP: he enthalpy (H)of vaporization of water is about seven times larger than water’s enthalpy...

See similar textbooks

Similar questions

The cooling effect of alcohol on the skin is due to its evaporation. Calculate the heat of vaporization of ethanol (ethyl alcohol), C2H5OH. C2H5OH(l)C2H5OH(g);H=? The standard enthalpy of formation of C2H5OH(l) is 277.7 kJ/mol and that of C2H5OH(g) is 235.1 kJ/mol.
What mass (g) of ethanol, CH3CH2OH(), can be vaporized at its boiling point of 78.4 C by transfer of 500. kJ to the liquid? The vapH of ethanol is 38.6 kJ/mol at this temperature.
he enthalpy (H)of vaporization of water is about seven times larger than water’s enthalpy fusion(41kJ/molvs.6kJ/mol). What does this tell us about the relative similarities among the solid, liquid, and gaseous states of water?
9.46 The heat of fusion of pure silicon is 43.4 kJ/mol. How much energy would be needed to melt a 5.24-g sample of silicon at its melting point of 1693 K?
The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.
Why does sweating cool the human body?
What is U when 1.00 mol of liquid water vaporizes at 100C? The heat of vaporization, Hvap, of water at 100C is 40.66 kJ/mol.
Follow the step-wise process outlined in Problem 31 to calculate the amount of heat involved in condensing 100.00 g of benzene gas (C6H6) at 80.00C to liquid benzene at 25.00C. Use Tables 8.1 and 8.2 for the specific heat, boiling point, and heat of vaporization of benzene.
Why are steam burns so much worse than water burns even if the H2O is at the same temperature for both phases? Hint: Consider the heat of vaporization of water.
6.25. Phosphorus exists as several allotropes that have varying properties. The enthalpy of transition from white P to red P, , is . The densities of white and red phosphorus are and , respectively. At what temperature does white phosphorus become the stable phase at of pressure? Assume the formula for phosphorus is .
How many grams of water at 0C will be melted by the condensation of 1 g of steam at 100C?
In regions with dry climates, evaporative coolers are used to cool air. A typical electric air conditioner is rated at 1.00 104 Btu/h (1 Btu, or British thermal unit = amount of energy to raise the temperature of 1 lb water by 1F). What quantity of water must be evaporated each hour to dissipate as much heat as a typical electric air conditioner?