Question

At 50.14 K a substance has a vapor pressure of 258.9 torr. Calculate its heat of vaporization in kJ/mol it if has a vapor pressure of 161.2 torr at 277.5 K.

Answer #1

**Answer** – Given, vapor pressure P_{1} =
258.9 torr, T_{1} = 50.14 K

T_{2} = 277.5 K , vapor pressure, P_{2} = 161.2
torr , ΔH_{vap} = ? kJ/mol

According to Clausius Clapeyron equation –

ln P_{1}/ P_{2} = ΔH_{vap} / R *(
1/T_{2} -1/T_{1})

ln 258.9 torr / 161.2 torr = ΔH_{vap} / 8.314
J.mol^{-1}.K^{-1} * ( 1/277.5 K – 1/50.14 K)

0.474 = ΔH_{vap} / 8.314
J.mol^{-1}.K^{-1} * -0.0163 K

**ΔH _{vap}**= 0.474 * 8.314 / -0.0163 K

= -241.1 J/mol

=
**-0.241 kJ/mol**

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