A hydrochloric acid solution $-$molar, $\{$:$SG1\mathrm{.}06,C_p=3\mathrm{.}35\frac{J}{gC}]$ 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$.$

Heat Removal

$$ Take reference states of $H_{2}O(l)$ 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

Attempts: unlimited

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$).$