Question

Use the Clausius equation to calculate the pressure in torr of a system at 300 K for ether knowing that the normal boiling point is 319 K and the delta H (the heat of vaporization) is 29.69 kJ/mol.

A. 403 torr
B. 120 torr
C. 1000 torr
D. 7 torr

Answer 1

To calculate the pressure in torr of a system at 300 K for ether, we can use the Clausius-Clapeyron equation.

Step-by-step explanation:

To calculate the pressure in torr of a system at 300 K for ether, we can use the Clausius-Clapeyron equation. The equation is given by: ln(P₁/P₂) = -ΔH/R (1/T₂ - 1/T₁), where P₁ is the vapor pressure at temperature T₁, P₂ is the vapor pressure at temperature T₂, ΔH is the heat of vaporization in J/mol, R is the gas constant (8.314 J/mol•K), and T₁ and T₂ are the temperatures in Kelvin.

Substituting the given values into the equation, we have ln(P₁/83.4 kPa) = -29.69 kJ/mol / (8.314 J/mol•K) (1/300 K - 1/319 K).

Calculating this expression gives us ln(P₁/83.4 kPa) = -0.647. Solving for P₁, we find P₁ = 83.4 kPa / e^(-0.647) ≈ 120 torr.