(a) In the lab, you have just prepared an unknown product, and you wish to characterize its physical properties. You find that its vapor pressure is 0.386 bar at 400 K, and that its normal boiling point is 432 K. Use the Clausius-Clapeyron equation to estimate the value of $ \Delta_{\text{vap}} \overline{H} $ for this compound in kJ.(b) With the information you have accumulated in part (a), now evaluate the molar entropy change, $ \Delta_{\text{vap}} \overline{S} $, for vaporization of your product, in J/K.(c) The vapor pressure of solid $ \text{I}_2 $ (iodine) is given by\[\ln(P) = -\frac{8090.0 \, K}{T} - 2.013 \ln(T) + 32.908\]where $ P $ is in atm and $ T $ is in K. Use this equation to compute the normal sublimation temperature, $ T_{\text{subl}} $ (in K). (*Note: It is best to use WolframAlpha or some numerical method, such as a Newton-Raphson iteration, to find the solution for this problem.*)

Answered: (a) In the lab, you have just prepared…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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(a) In the lab, you have just prepared an unknown product, and you wish to characterize its physical properties. You find that its vapor pressure is 0.386 bar at 400 K, and that its normal boiling point is 432 K. Use the Clausius-Clapeyron equation to estimate the value of $ \Delta_{\text{vap}} \overline{H} $ for this compound in kJ.

(b) With the information you have accumulated in part (a), now evaluate the molar entropy change, $ \Delta_{\text{vap}} \overline{S} $, for vaporization of your product, in J/K.

(c) The vapor pressure of solid $ \text{I}_2 $ (iodine) is given by

\[
\ln(P) = -\frac{8090.0 \, K}{T} - 2.013 \ln(T) + 32.908
\]

where $ P $ is in atm and $ T $ is in K. Use this equation to compute the normal sublimation temperature, $ T_{\text{subl}} $ (in K). (*Note: It is best to use WolframAlpha or some numerical method, such as a Newton-Raphson iteration, to find the solution for this problem.*)

Expert Solution

Step 1

Clausius-Clapeyron equation: This equation relates the vapor pressures at two different temperatures. And it is expressed as:

$\begin{array}{l} \ln (\frac{P_{1}}{P_{2}}) = \frac{{ΔH}_{vap}}{R} (\frac{1}{T_{2}} - \frac{1}{T_{1}}) \\ where \\ Δ H_{vap} is heat of vaporization \\ R is gas constant \\ P_{1} is pressure at temperature T_{1} \\ P_{2} is pressure at temperature T_{2} \end{array}$

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