Assuming $\Delta$H° and $\Delta$S° are temperature independent, calculate the normal boiling point of bromine.

Question

Quizplus · Accepted Answer

The given equation is a thermochemical equation for the formation of Br2 from its elements in their standard states. The standard state of Br2 is a liquid at 1 atm and the standard enthalpy of formation of Br2 is -30.91 kJ/mol. Using the Clausius-Clapeyron equation, we can relate the boiling point of a substance to its enthalpy of vaporization, temperature, and pressure. The equation is ln(P2/P1) = ΔHvap/R [(1/T1) - (1/T2)]. We can use this equation to calculate the normal boiling point of Br2 (i.e. boiling point at 1 atm).

Let's assume the normal boiling point of Br2 is T2. At the normal boiling point, the vapor pressure of Br2 is equal to atmospheric pressure (i.e. 1 atm). Therefore, we can rewrite the Clausius-Clapeyron equation as ln(1/1) = ΔHvap/R [(1/T1) - (1/T2)].

Simplifying for T2, we get T2 = ΔHvap/R [(1/T1) - ln(1)]^-1.

Plugging in the values, we get T2 = (-30.91 kJ/mol)/(8.314 J/mol∙K) [(1/298 K) - (1/373 K)]^-1 = 332 K.

Therefore, the normal boiling point of Br2 is 332 K, which is equivalent to 59°C. The answer is D) 332 K.

Assuming Δ\DeltaΔ H° And Δ\DeltaΔ S° Are Temperature Independent, Calculate the Normal Boiling Point of the Normal

Assuming $\Delta$ H° And $\Delta$ S° Are Temperature Independent, Calculate the Normal Boiling Point of the Normal