A dilute solution of bromine in carbon tetrachloride behaves as an ideal-dilute

Question

A dilute solution of bromine in carbon tetrachloride behaves as an ideal-dilute solution. The vapour pressure of pure CCl4 is 33.85 Torr at 298 K. The Henry's law constant when the concentration of Br2 is expressed as a mole fraction is 122.36 Torr. If the mole faction of Br2 is 0.02,and the conditions of the ideal-dilute solution are satisfied at this concentration, calculate the vapour pressure of each component P(CCl4, Torr)= ________? , P(Br2, Torr)= _________?, the total pressure P(total, Torr)= __________?, and the composition of the vapour phase y(CCl4)= ________? and y(Br2)= ________?.

Explanation / Answer

total pressure = 33.85 + 122.36 = 156.21 torr

P (Br2) = mole fraction x total pressure = 0.02 x 156.21 = 3.12 torr

P (CCl4) = mole fraction of CCl4 x total pressure = 1.02 x 156.21 = 153.1 torr

mole fraction of Br2 x partial pressure = mole fraction in vapoure phase x total pressure

0.02 x 3.12 = mole fraction in vapoure phase x 156.31

mole fraction in vapoure phase (Br2) = 0.00399

mole fraction of CCl4 x partial pressure = mole fraction in vapoure phase x total pressure

0.92 x 153.1 = mole fraction in vapoure phase x 156.31

mole fraction in vapoure phase (CCl4) = 0.901 torr

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.