Substance X has a heat of vaporization of 58.4 kJ/mol at its normal boiling point (423°C).For the process X(l)$\to$X(g)at 1 atm and 423°C calculate the value of $\Delta$S_surr.

Question

Quizplus · Accepted Answer

The entropy change of the surroundings (ΔS_surr) is calculated using the formula ΔS_surr = -ΔH/T, where ΔH is the heat of vaporization and T is the temperature in Kelvin. Converting 423°C to Kelvin gives 696 K. Thus, ΔS_surr = -58,400 J/mol / 696 K = -83.9 J/K mol.

Substance X Has a Heat of Vaporization of 58 →\to→ X(g)at 1 Atm and 423°C Calculate the Value Of

Substance X Has a Heat of Vaporization of 58 $\to$ X(g)at 1 Atm and 423°C Calculate the Value Of