Question

3 pts Question 13 What is the vapor pressure of a pure sample of butanal at 50°C? The normal boiling point is 75.7°C and the heat of vaporization is 34.2 kJ/mol. O 760 torr 481 torr O 297 torr 098 torr

Answer 1

Hi there,

For this question we have to use Clausius Clapeyron Equation

1 1 ---6--] 1 P1 & P2 = Initial & Final Pressure : AvapHm = Molar Enthalpy of vaporization ; T1, T2 = Initial & Final Temperature ; R=Gas Constant;

P₁ = 1atm = 760 mmHg = 760 torr

T₁ = 75.7 ⁰C = 75.7 + 273 = 348.7 K,

T₂ = 50 ⁰C = 50 + 273 = 323 K

Δ_vapH_m = Molar Enthalpy of vaporization = 34.2 kJ/mol;

R = 0.0083145 J/mol.K

P₂ = to be calculated

by substituting above values in equation, we get

P₂ = 297.533512766373 torr ~ 297 torr

Answer: 297 torr

3 pts Question 13 What is the vapor pressure of a pure sample of butanal at 50°C? The normal boiling point is 75.7°C and the heat of vaporization is 34.2 kJ/mol. 760tor G 481 torr 297 torr 98 topp-

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