High School

We appreciate your visit to The vapor pressure of ethanol is 450 mmHg at 68 5 C Its molar heat of vaporization is 39 3 kJ mol What is the. This page offers clear insights and highlights the essential aspects of the topic. Our goal is to provide a helpful and engaging learning experience. Explore the content and find the answers you need!

The vapor pressure of ethanol is 450 mmHg at 68.5°C. Its molar heat of vaporization is 39.3 kJ/mol. What is the vapor pressure of ethanol, in mmHg, at 40.9°C?

Answer :

Final Answer:

The vapor pressure of ethanol at 40.9°C is approximately 262.2 mmHg.

Explanation:

The relationship between vapor pressure and temperature is described by the Clausius-Clapeyron equation:

ln(P₂/P₁) = -ΔHvap / R x (1/T₂ - 1/T₁)

Where:

P₁ = vapor pressure at temperature T₁

P₂ = vapor pressure at temperature T₂

ΔHvap = molar heat of vaporization

R = ideal gas constant (8.314 J/mol·K)

T₁ = initial temperature in Kelvin

T₂ = final temperature in Kelvin

Given that P₁ = 450 mmHg at

T₁ = 68.5°C = 341.65 K, and

ΔHvap = 39.3 kJ/mol, we want to find P₂ at

T₂ = 40.9°C = 314.05 K.

Converting ΔHvap to joules/mol:

ΔHvap = 39.3 kJ/mol x 1000 J/kJ

= 39300 J/mol

Plugging the values into the Clausius-Clapeyron equation:

ln(P₂/450) = -39300 / (8.314 x (1/314.05 - 1/341.65))

Solving for P₂:

P₂ = 450 x e^(-39300 / (8.314 x (1/314.05 - 1/341.65)))

P₂ ≈ 262.2 mmHg

Therefore, the vapor pressure of ethanol at 40.9°C is approximately 262.2 mmHg.

Learn more about Vapor pressure

brainly.com/question/32773821

#SPJ11

Thanks for taking the time to read The vapor pressure of ethanol is 450 mmHg at 68 5 C Its molar heat of vaporization is 39 3 kJ mol What is the. We hope the insights shared have been valuable and enhanced your understanding of the topic. Don�t hesitate to browse our website for more informative and engaging content!

Rewritten by : Barada