Determine the normal boiling point of a substance whose vapour pressure is 73.46 mbar at 35 °C and has a Δ_vapH of 32.1 kJ mol^-1. A) 255 K B) 368 K C) 412 K D) 390. K E) 466 K

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The Clausius-Clapeyron equation is:ln(P₂/P₁) = -Δ_vapH/R * (1/T₂ - 1/T₁)where P₁ and T₁ are the initial pressure and temperature, P₂ and T₂ are the final pressure and temperature, Δ_vapH is the enthalpy of vaporization, and R is the gas constant.We can rearrange this equation to solve for T₂:T₂ = Δ_vapH/R * (1/T₁ - ln(P₂/P₁))Plugging in the given values, we get:T₂ = 32.1 kJ mol^-1 / (8.314 J mol^-1 K^-1) * (1/308 K - ln(73.46 mbar / 1013 mbar))T₂ = 390. K

Determine the Normal Boiling Point of a Substance Whose Vapour