A certain substance has a heat of vaporization of 57.85kJ/mol. At what kelvin te

Question

A certain substance has a heat of vaporization of 57.85kJ/mol. At what kelvin temperature will the vapor pressure be 4.00 times higher than it was at 307 K?
I need help solving and working through this problem. Please help. A certain substance has a heat of vaporization of 57.85kJ/mol. At what kelvin temperature will the vapor pressure be 4.00 times higher than it was at 307 K?
I need help solving and working through this problem. Please help.
I need help solving and working through this problem. Please help.

Explanation / Answer

Solution is as below.

We will use the Calusius-Clapeyron equation

ln(P1/P2) = delta Hvap/R [1/T2 - 1/T1]

we have,

P1 (initial vapor pressure) = 1

P2 (final vapor pressure) = 4

T1 (initial temperature) = 307 K

T2 (final temperature) = unknown

delta Hvap = 57.85 kJ/mol = 57850 J/mol

R = (gas constant) 8.314 J/mol.K

Feeding the values we get,

ln(1/4) = (57850/8.314)[(1/T2) - (1/307)]

T2 = 327 K

Thus, at 327 K the vapor pressure will be 4.00 times higher than it was at 307 K.

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