Chm 2046

posted by .

The normal boiling point of liquid ethanol is 351 K. Assuming that its molar heat of vaporization is constant at 37.5 kJ/mol, the boiling point of C2H5OH when the external pressure is 1.35 atm is K.

  • Chm 2046 -

    Use the Clausius-Clapeyron equation.
    You know p = 1 atm when T = 351K. Solve for p2 when T = 1.35 atm.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. apchem

    A 15.0g sample of liquid ethanol, C2H5OH, absorbs 5.13x10^3 J of heat at its normal boiling point, 78.0C. The molar enthalpy of vaporization of ethanol is 39.3kJ/mol. (a) What volume of ethanol vapor is produced?
  2. Chemistry

    A 15.0g sample of liquid ethanol, C2H5OH, absorbs 5.13x10^3 J of heat at its normal boiling point, 78.0C. The molar enthalpy of vaporization of ethanol is 39.3kJ/mol. (a) What volume of ethanol vapor is produced?
  3. chemistry

    How much heat is required to vaporize 3.50L of at its normal boiling point?
  4. chemistry

    How much heat is required to vaporize 3.50L of at its normal boiling point?
  5. Chemistry

    The following information is given for ethanol, C2H5OH, at 1atm: boiling point = 78.4oC Hvap(78.4oC) = 38.6 kJ/mol melting point = -115oC Hfus(-115oC) = 5.02 kJ/mol specific heat liquid = 2.46 J/goC At a pressure of 1 atm, what is …
  6. Chemistry

    In one experiment, the mass of water is 92.6 grams, the initial temperature of the water is 67.6oC, the mass of liquid nitrogen added to the water is 61.4 grams, and the final temperature of the water, after the liquid nitrogen has …
  7. Chemistry

    Neat pure ethanol C2H5OH has an enthalpy of vaporization of 39.3 Kj/mol, and a vapor pressure of 0.308 atm at 50 C. What is the boiling point, at atmospheric pressure of 1 atm, of a solution consisting of 35 G of phenol (a non-electrolyte …
  8. Chemistry

    Ethanol (C2H5OH) has been produced since antiquity by the fermentation of fruits and vegetables. Given the following data, if 5.87 kJ of energy are transferred to 13.3 g of frozen ethanol at -130.0 °C, what is the final temperature …
  9. Chemistry

    The equation for the best fit line was y = -4058.7x + 16.10. Using the equation of the best fit line, calculate the heat of vaporization (delta H) and the NORMAL BOILING POINT (in Celsius) of this volatile liquid. Calculated: dHvap …
  10. chemistry

    The following information is given for ether, C2H5OC2H5, at 1atm: boiling point = 34.6 °C Hvap(34.6 °C) = 26.5 kJ/mol specific heat liquid = 2.32 J/g°C At a pressure of 1 atm, kJ of heat are needed to vaporize a 41.0 g sample of …

More Similar Questions