A certain substance has a heat of vaporization of 39.90 kJ/mol. At what Kelvin temperature will the vapor pressure be 5.50 times higher than it was at 325 K?
Given:
Delta Hvap = 39.90 kJ/mol = 39900 J /mol
Vapor pressure of substance is 5.50 time higher than that of the vapor pressure at 325 K
Solution:
We use Classius clapeyron equation to get temperature at which the pressure is 5.50 times.
Equation:
Ln (p2/p1) = (-Delta H/R) x ( 1/T2-1/T1)
Here p2 is the vapor pressure at Temperature T2, P1 is vapor pressure at temperature T1.
Lets P2/p1 = 5.50
Delta H = heat of vaporization in J /mol , R = 8.314 J / (K mol ) , T is in Kelvin.
Let T1 = 325 K.
Lets plug all the values to get T2.
Ln (5.50) = (- 39900 / 8.314 ) x ( 1/T2 - 1/ 325 )
T2 = 367.42 K
The temperature of the substance will be = 367.42 K
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