Respuesta :
Answer:- The pressure of ethanol would be 109 mmHg.
Solution:- This problem is based on Clausius clapeyron equation--
[tex]ln(\frac{P_1}{P_2})=(\frac{\Delta Hvap}{R})(\frac{1}{T_2}-\frac{1}{T_1})[/tex]
Given, [tex]T_1[/tex] = 63.5 + 273 = 336.5 K
[tex]T_2[/tex] = 34.9 + 273 = 307.9 K
[tex]P_1[/tex] = 400 mmHg
[tex]P_2[/tex] = ?
[tex]\Delta Hvap[/tex] = 39.3 kJ/mol = 39300 J/mol
R = 8.314 J/mol.K
Let's plug in the values in the equation and do the calculations.
[tex]ln(\frac{400}{P_2})=(\frac{39300}{8.314})(\frac{1}{307.9}-\frac{1}{336.5})[/tex]
[tex]ln(\frac{400}{P_2})[/tex] = 1.30
On taking anti ln to both sides...
[tex]\frac{400}{P_2}[/tex] = [tex]e^1^.^3^0[/tex]
[tex]\frac{400}{P_2}[/tex] = 3.67
[tex]P_2[/tex] = 400/3.67
[tex]P_2[/tex] = 109 mmHg
The study of chemicals is called chemistry. The weight of every element in the compound is called molecular mass.
The correct answer to the question is 109mmhg.
What is vapor pressure?
- Vapor pressure or equilibrium vapor pressure is defined as the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature in a closed system.
- The equilibrium vapor pressure is an indication of a liquid's evaporation rate.
The formula used to solve the question is :-
[tex]In\frac{P_1}{P_2}=\frac{H_{vap}}{R}(\frac{1}{T_2} -\frac{1}{T_1} )[/tex]
The data is given as follows:-
- T = 63.5 + 273 = 336.5 K
- T= 34.9 + 273 = 307.9 K
- P = 400 mmHg
Place all the values in the question.
[tex]In\frac{400}{P_2} =\frac{39300}{8.314} (\frac{1}{307.9} -\frac{1}{336.5} )\\\\\frac{400}{P_2} =1.30\\\\P_2=109mmhg[/tex]
Hence, the correct answer to the question is 109.
For more information about the question, refer to the link:-
https://brainly.com/question/1453843
