A hydrochloric acid solution $[4-$molar, SG $1\mathrm{.}06,C_p=3\mathrm{.}35\frac{J}{gC}]$ is produced by absorbing hydrogen chloride $HCl(g)$ in water.

Liquid water enters the absorber at $35\mathrm{.}0C$ and gaseous $HCL$ is fed at $20\mathrm{.}0C$ and $790\mathrm{.}0$ torr absolute$.$

Essentially all of the HCL fed to the column is absorbed$.$

Take one liter of product solution as a basis of calculation.

Physical Property Tables

Volume of $HCL$

Correct.

Estimate the volume $($liters$)$ of HCL that must be fed to to the absorber$.$

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Hint

Attempts: $1$ of $3$ used

Heat Removal

Take reference states of $H_{2}O(I)$ and $HCl(g)$ at $25C.$

Estimate the heat $(kJ)[$absolute value$]$ that must be transferred from the absorber if the product solution is to emerge at $50\mathrm{.}0C.$ kJ $($positive$)$

Hint

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Attempts: $1$ of $3$ used

Adiabatic Operation

It is easy to get confused with signs in these sorts of problems.

Estimate the final solution temperature if the absorber operates adiabatically $($if it did not boil first$).$

$C$

Hint

Assistance Used

For adiabatic operation, $Q=0.$