Determine $\Delta$H_f^{$\omicron $}(HCl(g)) from the following data. H-Cl bond enthalpy = +431 kJ.mol^-¹ $\Delta$H_f^{$\omicron $(}H(g))= +217.9 kJ.mol^-¹ $\Delta$H_f^{$\omicron $}(Cl(g))= +121.4 kJ.mol^-¹ A) +92 kJ.mol^-¹ B) -261 kJ.mol^-¹ C)-431 kJ.mol^-¹ D) +431 kJ.mol^-¹ E) -92 kJ.mol^-¹

Question

Quizplus · Accepted Answer

The formation enthalpy of HCl(g) can be calculated using the equation: $\Delta$H_f^{$\omicron $}(HCl(g)) = $\Delta$H_f^{$\omicron $}(H(g)) + $\Delta$H_f^{$\omicron $}(Cl(g)) - H-Cl bond enthalpy. Substituting the given values: 217.9 + 121.4 - 431 = -91.7 kJ/mol, which rounds to -92 kJ/mol.

Determine Δ\DeltaΔ Hf ο\omicron ο (HCl(g)) from the Following Data Δ\DeltaΔ Hf ο\omicron ο

Determine $\Delta$ H_f^$\omicron$(HCl(g)) from the Following Data $\Delta$ H_f^$\omicron$