The vapor pressure, ?P, of a certain liquid was measured at two temperatures, ?T. The data is shown in the table.
T (K) | P (kPa) |
---|---|
225 | 3.75 |
825 | 6.26 |
Keep the pressure units in kPa.
If you were going to graphically determine the enthalpy of vaporizaton, Δ?vapΔHvap, for this liquid, what points would you plot? To avoid rounding errors, use three significant figures in the x-values and four significant figures in the y-values.
point 1: x=
point 1: y=
point 2: x=
point 2: y=
Determine the rise, run, and slope of the line formed by these points.
Rise =
Run =
Slope =
What is the enthalpy of vaporization of this liquid? In J/mol.
We need to plot lnP on y axis and 1/T on x axis
P = 3.75
ln P = ln (3.75) = 1.32176
T = 225.0
1/T = 0.00444
point 1 is:
x = 0.00444
y = 1.32176
P = 6.26
ln P = ln (6.26) = 1.83418
T = 825.0
1/T = 0.00121
point 2 is:
x = 0.00121
y = 1.83418
----------------------------------------------------------------------------
rise = (y1-y2) = 1.32176 - 1.83418 = -0.51242
rise = (X1-X2) = 0.00444 - 0.00121 = 0.00323
slope = rise/run
= -0.51242/0.00323
= -158.53128
----------------------------------------------------------------------------
use
slope = - HVap/R
-158.53128 = -HVap/8.314
HVap = 1318 J/mol
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