Chemistry - Thermodynamics - II Question with Solution | TestHub

In a hypothetical universe, ${\mathrm{H}}_3{\mathrm{BO}}_3(\mathrm{s})$ obtained from the following reaction is completely sublimed at 300 K.

${\mathrm{B}}_2{\mathrm{H}}_6(\mathrm{g})+6{\mathrm{H}}_2\mathrm{O}(\mathrm{l})\to 2{\mathrm{H}}_3{\mathrm{BO}}_3(\mathrm{s})+6{\mathrm{H}}_2(\mathrm{g})$.

The necessary energy for sublimation was obtained through work released by one cycle of an ideal heat engine in which one mole of monoatomic perfect gas flows through the cycle described in the pressure (p) – volume (V) diagram below.

* A→B; isothermal reversible expansion receiving 250 J by heat transfer ($q_H$) at a temperature of 1000 K ($T_H$) from a hot source.

* B→D; reversible adiabatic expansion.

* D→C; isothermal reversible compression at a temperature of 300 K ($T_C$) releasing some amount of heat ($q_C$) to a cold sink.

* C→A; reversible adiabatic compression.

Calculate the amount of H₂(g) (mg) produced according to the reaction. The enthalpy of sublimation of H₃BO₃(s) is 25.00 KJ/mol.