The vapor pressure of ethanol is 1.00 x 102 mmHg at 34.90oC. What is its vapor...
The vapor pressure of ethanol is 1.00 x 102 mmHg at 34.90oC. What is its vapor pressure at 51.73 oC? (ΔHvap for ethanol is 39.3 Kj/mol.)
Given the vapor pressure at one temperature, P1, we can calculate the vapor pressure at a second temperature, P2.
In (P1/P2) = ΔHvap/R (1/T2 - 1/T1)
Where,
ΔHvap for ethanol must have the units of J/mol.
R = 8.314 J/K.mol .. The temperatures must be in Kelvins.
Solve for P2, What is the vapor pressure of ethanol at 51.73 oC?
Homework Answers
The relation between the vapor pressure and temperature can be expressed by an equation called Clausius–Clapeyron equation. Vapor pressure of substances can be calculated by using this equation.
Clausius–Clapeyron equation:-
Here
Conversion factor;
Given,
Given,
Substitute the given values in Clausius–Clapeyron equation for finding 
,
The vapor pressure of the ethanol at 
is 
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