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P1 = 760 torr

P2 = 83 torr

T1 = ?

T2 = -170 degrees C + 273 = 103 K

delta H = 7.50 kJ/mole x (1000 J / 1 kJ) = 7,500 J/mole

R = 8.314 K/J/mole

ln (P2 / P1) = - (delta H / R) x (1/T2 - 1/T1)

ln (83 torr / 760 torr) = - (7,500 J/mole / 8.314 K/J/mole) x (1/103 K - 1/T1)

T1 = 137.85658472 K

T1 = 137.85658472 K - 273.15 K = -135.29

T1 = -135 degrees C

Ex.

  • Maybe can use (?): T2 = [ 1/T1 - (( R x ln(P2/P1) / delta H)) ]-1

Screen Reader Note: To calculate percent error, find the absolute value of the difference between experimental value and known value. Take this and divide it the known value. After that, multiply by 100 %. End of note.

Given the known heat of vaporization (delta H vap) of water is 44.01 kJ/mole, find the percent error using the experimentally determined delta H vap of 43.97 kJ/mole. Express with units of % in the units box.

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An unknown liquid has a heat of vaporization of 34.13 kJ/mole. If the normal boiling point is 82, what is vapor pressure (in torr) of this liquid at room temperature of 25 degrees C? HINT: Normal boiling point occurs when the vapor pressure of the liquid is the same as atmospheric pressure (1 atm or 760 mm Hg).

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An unknown liquid has a heat of vaporization of 7.50 kJ/mole. If the vapor pressure of this liquid at -170 degrees C is 83 torr, what is the normal boiling point of this liquid in degrees C? HINT: Normal boiling point occurs when the vapor pressure of the liquid is the same as atmospheric pressure (1 atm or 760 mm Hg).

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