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3. Saturate vapor pressure of pure C&H=C1(1) and pure C6H5Br(1) are 125238 Pa and 66104 Pa, respectively. Assuming that the i

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Solution:​​​​

Let subscript 'A' stand for C6H5Cl

Let subscript 'B' stands for C6H5Br

Given Presure, P = 1 atm = 101325 Pa

Given bubble point temperature, T= 413.2 K

Vapor Pressure of C6H5Cl, P​​​​​​​​​​​​s​​​​​A= 125238 Pa

Vapor Pressure of C6H5Br,  P​​​​​​s​​​​​​​​​​B = 66104 Pa

The composition of the first vapour produced from a liquid of boiling is calculated as follows.

We know Total pressure is the sum of partial pressures (Dalton's Law)

P = p​​​​​​A + p​​​​​​B

where   p​​​​A ​​​​​​= partial pressure of C6H​​​​​​​​​​​​6Cl

p​​​​​​B = partial pressure of C6H5Br

We know  p​​​​​​A = X​​​​​​A * P​​​​​​s​​A ------ ( Raoult's law )

Similarly p​​​​​​B = X​​​​​B  * P​​​​​​sB

Where X​​​​​​Ais the mole fraction of C6H5Cl in liquid mixture and X​​​​​​B is the mole fraction of C6H​​​​5​​​Br in liquid mixture.

P = X​​​​​A * P​​​​​​sA + X​​​​​​​B * PsB

P= X​​​​​​A * P​​​​​​s​​​​​A + (1-XA) * P​​​​​​sB

Therefore X​​​​​​A = (P - P​​​​​​s​​​​​B) / ( P​s​​​​A - P​sB)

X​​​​​​A = (101325 - 66104) / (125238 - 66104) = 0.5956

X​​​​​B = 1 - X​​​​​​A = 1 - 0.5956 = 0.4044

By Applying Dalton's Law, the partial pressure of component gas is in an ideal gas mixture is the product of its mole fraction and the total pressure.

​​​​​​y​​​​​​A = p​​​​​​A / P

y​​​​​​B = p​​​​​​B / P

Where y​​​​​​Aand y​​​​​​Bare the mole fraction of C6H5Cl and C6H5Br respectively.

y​​​​​​A =( XA * P​​​​​​s​A ) / P

y​​​​​​A = (0.5956 * 125238) / 101325 = 0.7362

y​​​​​​B = 1 - y​​​​​​A = 1 - 0.7362 = 0.2638

VAPOR COMPOSITION

C6H5Cl = 73.62%

C6H6Br = 26.38%

LIQUID COMPOSITION

C6H5Cl = 59.56%

C6H5Br = 40.44%

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