Respuesta :
Answer: The total vapor pressure of the solution is 81.3 mmHg
Explanation:
To calculate the total pressure, we use the equation given by Dalton and Raoults, which is:
[tex]p_T=(p_A\times \chi_A)+(p_B\times \chi_B)[/tex]
where,
[tex]p_T[/tex] = total vapor pressure
We are given:
Mole fraction of benzene = 0.580
Mole fraction of toluene = (1 - 0.580) = 0.420 (Total mole fraction is always equation to 1)
Vapor pressure of benzene = 183 mmHg
Vapor pressure of toluene = 59.2 mmHg
Putting values in above equation, we get:
[tex]p_T=(183\times 0.580)+(59.2\times 0.420)\\\\p_T=81.3mmHg[/tex]
Hence, the total vapor pressure of the solution is 81.3 mmHg
The total vapor pressure of the given solution of toluene and benzene has been 131.004 mm Hg.
From Dalton's law of vapor pressure:
Total Vapor pressure = mole fraction of A [tex]\times[/tex] Vapor pressure of a + mole fraction of B [tex]\times[/tex] Vapor pressure of B.
Given, the mole fraction of Benzene = 0.580.
The sum of mole fractions in a solution has been 1.
1 = mole fraction of bemzene + mole fraction of toluene
1 = 0.580 + mole fraction of toluene
Mole fraction of toluene = 1 - 0.580
Mole fraction of toluene = 0.420
Total pressure = (0.580 [tex]\times[/tex] 183) + (0.420 [tex]\times[/tex] 59.2) mm Hg
Total pressure = 106.14 + 24.864 mm Hg
Total vapor pressure = 131.004 mm Hg.
The total vapor pressure of the given solution of toluene and benzene has been 131.004 mm Hg.
For more information about the vapor pressure, refer to the link:
https://brainly.com/question/25356241
