AP CHEM

2-propanol has a delta Hvp of 701 J/g and a vapor pressure of 31.6 mmHg at 20.0 degrees C. Estimate the normal boiling point of this alcohol in degrees C.

i used the clasius-clayperon equation and this is what i have so far.

ln (31.6 mmHg/760 mmHg)= (-701 J/g)/8.314 J/g C (1/ T2 - 1/20 C)

is that correct?

  1. 👍
  2. 👎
  3. 👁
  1. No, you have at least two errors. T must be converted to Kelvin and Hvap must be in J/mol. Therefore, T1 = 273.15 + 20.0 = ?? and Hvap for 2-propanol is 701 J/g x ??grams/mol = ??

    1. 👍
    2. 👎
  2. Also, I think the equation should be ln(p2/p1). You have reversed the T1 and T2 but that is ok since you have a negativae sign for Hvap. But P2 should be on top and P1 on bottom.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    the vapor pressure of water at 45.0 °c is 71.93 mmhg. Calculate the vapor pressure of a solution of 1.50 m Al(NO3)3 at this temperature (assume 100% dissociation)

  2. Chemistry

    The vapor pressures of ethanol (C2H5OH) and 1-propanol (C3H7OH) are 100 mmHg and 37.6 mmHg, respectively. Assume ideal behavior and calculate the partial pressures of ethanol and 1-propanol at 35 degrees Celsius over a solution of

  3. Chemistry

    Given that the vapor pressure of water is 17.54 torr at 20 C, calculate the vapor-pressure lowering of aqueous solutions that are 2.40 m in (a) sucrose, C12H22O11, and (b) aluminum chloride. Assume 100% dissociation for

  4. chemistry 1B

    1-propanol (P1° = 20.9 Torr at 25 °C) and 2-propanol (P2° = 45.2 Torr at 25 °C) form ideal solutions in all proportions. Let x1 and x2 represent the mole fractions of 1-propanol and 2-propanol in a liquid mixture,

  1. chemistry

    Calculate the vapor pressure lowering of water when 5.67 g of glucose, C6H12O6, is dissolved in 25.2 g of water at 25 ºC. The vapor pressure of water at 25º C is 23.8 mmHg. What is the vapor pressure of the solution?

  2. Chemistry

    Equilibrium is established between Br2(l) and Br2(g) at 25.0*C. A 250.0 mL sample of the vapor weights 0.486g. What is the vapor pressure of bromine at 25.0*C, in mmHg?

  3. Chemistry

    The vapor pressure of pure ethanol at 20 degrees C is 44 mmHg, and the vapor pressure of pure methanol at the same temperature is 94 mmHg. In a solution of the two, the mole fraction of ethanol is .439; the mole fraction for

  4. chemistry

    The Vapor pressures of pure propyl alcohol and isopropyl alcohol are 21.0 mmHg and 45.2 mmHg, respectively, at 25 (degrees)C. Calculate the partial pressure of isopropyl alcohol above a solution in which the mole fraction of

  1. chem

    The reaction AB(aq)->A(g)+ B(g)is second order in AB and has a rate constant of 0.0282 M^{-1} s^{-1} at 25 Celsius. A reaction vessel initially contains 250 mL of 0.105 M AB which is allowed to react to form the gaseous product.

  2. Chemistry

    Please help! The vapor pressure of water at 35 oC is 42.175 mm Hg. The vapor pressure of ethyl alcohol (C2H5OH) at 35 C is 100.5 mm Hg. What is the vapor pressure of a solution prepared by dissolving 250 g of C2H5OH in 375 g of

  3. chemistry

    the vapor pressure of ethanol at 20c is 44 mmHg and the vapor pressure of methanol at the same temperature is 94mmHg. A mixture of 30.0 g of methanol and 45.0 g of ethanol is prepared (and can be assumed to behave as an ideal

  4. chemistry

    the vapor pressure of pure water at 60 c is 157 mmHg. what is the vapor pressure of this solution at the same temperature, in mm Hg?

You can view more similar questions or ask a new question.