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Komok [63]
3 years ago
12

The vapor pressure of liquid chloroform, CHCl3, is 400.0 torr at 24.1 °C and 100.0 torr at –6.3 °C. What is DeltaH of vaporizati

on for chloroform?
Chemistry
1 answer:
Kryger [21]3 years ago
4 0

Answer:

ΔH vaporization of chloroform is 30.1kJ/mol

Explanation:

It is possible to find ΔH of vaporization of certain compound knowing vapor pressure under 2 different absolute temperatures (In Kelvin) by using Clausius-Clapeyron equation:

ln\frac{P_2}{P_1}=\frac{DeltaHvap}{R}  (\frac{1}{T_1} - \frac{1}{T_2} )

<em>Where P is vapor pressure. R is gas constant (8.314J/molK) and T absolute temperature of 1, first state and 2, final state.</em>

Absolute temperatures in the problem are:

T₁ = 24.1°C + 273.15 = 297.25K

T₂ = -6.3°C + 273.15 = 266.85K

Replacing:

ln\frac{P_2}{P_1}=\frac{DeltaHvap}{R}  (\frac{1}{T_1} - \frac{1}{T_2} )

ln\frac{100torr}{400.0torr}=\frac{DeltaHvap}{8.314J/molK}  (\frac{1}{297.25K} - \frac{1}{266.85K} )

ln\frac{100torr}{400.0torr}={DeltaHvap}* -4.6x10^{-5}mol/J

30073J/mol = 30.1kJ/mol = ΔHVap

<h3>ΔH vaporization of chloroform is 30.1kJ/mol</h3>
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