The heat of vaporization is the heat required to turn 1 gm solid into a liquid. The vapor pressure of diethyl ether at 76 degrees celsius is 1.95 atm.
Vapour pressure is the pressure exerted by the vapors of the equilibrium system. Clausius-Clapeyron equation is used to find the vapor pressure.
[tex]\rm ln \dfrac{P_{2}}{P_{1}} = \rm \dfrac{\delta H}{R} (\dfrac{1}{T_{1}} - \dfrac{1}{T_{2}})[/tex]
Given,
Initial pressure = 0. 703 atm
Initial temperature = 298K
Final temperature = 349 K
Change in enthalpy of vaporization = 29100J/mol
Boltzman constant = 8.314 J/K mol
Substituting values above:
[tex]\begin{aligned} \rm ln \dfrac{P_{2}}{P_{1}} & = \rm \dfrac{\delta H}{R} (\dfrac{1}{T_{1}} - \dfrac{1}{T_{2}})\\\\&= \dfrac{9100}{8.314}(0.0004903)\\\\&= 0.5363\end{aligned}[/tex]
Solving further,
[tex]\begin{aligned} \rm ln \dfrac{P_{2}}{0.703} &= 0.5363\\\\& = \rm e^{0.5363}\\\\&= 1.70\end{aligned}[/tex]
The final pressure is calculated as:
[tex]\rm P_{2} = (0.703 atm)(1.70) = 1.95\;\rm atm[/tex]
Therefore, the vapor pressure at 76 degrees celsius is 1.95 atm.
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