The vapor pressure of ethanol is 1.00 × 102 mmHg at 34.90°C. What is its vapor pressure at 60.61°C? (ΔHvap for ethanol is 39.3 kJ/mol.) mmHg

The vapor pressure of ethanol at 60.61 °C is 327.56 mmHg

Explanation:

using Clausius-Clapeyron equation

where;

ΔH is the enthalpy of vaporization of ethanol = 39.3 kJ/mol

R is ideal gas constant = 8.314 J/mol.K

P₁ is the initial pressure of ethanol at T₁ =  1.00 × 10² mmHg

P₂ is the final pressure of ethanol at T₂ = ?

T₁ is the initial temperature = 34.9°C = 307.9 K

T₂ is the final temperature = 60.61°C = 333.61 K

Therefore, the vapor pressure of ethanol at 60.61 °C is 327.56 mmHg

a=d/t

a="triangle"v/t

explanation:

a = acceleration