Answer:
To calculate the dew-point temperature and the composition of the liquid at the dew-point for the equimolar mixture of carbon tetrachloride (CCl4) and cyclohexane (C6H12), we need to use the Antoine equation and Raoult's law.
Calculate the vapor pressures of CCl4 and C6H12 at the given temperature using the Antoine equation:
For CCl4:
log10(P1) = A - (B / (T + C))
The Antoine equation constants for CCl4 are:
A = 13.232
B = 2949.2
C = -48.49
For C6H12:
log10(P2) = A - (B / (T + C))
The Antoine equation constants for C6H12 are:
A = 13.781
B = 2756.22
C = -47.48
Apply Raoult's law to determine the partial pressures of the components in the vapor phase:
P1* = x1 * P1
P2* = x2 * P2
where P1* and P2* are the partial pressures of CCl4 and C6H12 in the vapor phase, respectively, and x1 and x2 are the mole fractions of CCl4 and C6H12 in the liquid phase.
Use the total pressure and the partial pressures to calculate the mole fractions of the components in the vapor phase:
y1 = P1* / P_total
y2 = P2* / P_total
where y1 and y2 are the mole fractions of CCl4 and C6H12 in the vapor phase, respectively.
The dew-point temperature is the temperature at which the vapor phase is in equilibrium with the liquid phase. At the dew-point, the mole fractions of the components in the vapor phase are equal to the mole fractions of the components in the liquid phase:
y1 = x1
y2 = x2
Solve these equations to find the mole fractions of CCl4 and C6H12 in the liquid phase at the dew-point.
Note: The actual calculations require specific values for temperature, but they have not been provided in the question. Therefore, the exact values for the dew-point temperature and the composition of the liquid at the dew-point cannot be determined without knowing the specific temperature