Question

In: Chemistry

the vapor pressure of pure carbon disulfide and carbon tetrachloride are 360. and 99.8 torr, respectively,...

the vapor pressure of pure carbon disulfide and carbon tetrachloride are 360. and 99.8 torr, respectively, at 298K. What is the (total vapor pressure of a solution containing 50.0g of each compound A. 460. torr B. 274 torr C 260. torr D. 33.0 torr E. 241 torr

Solutions

Expert Solution

Answer- Given, vapor pressure of CS2 = 360 torr, for CCl4 = 99.8 torr

Mass of CS2 = 50.0 g and mass of CCl4 = 50.0 g

Now we need to calculate the moles of each

Moles of CS2 = 50.0 g / 76.143 g.mol-1 = 0.657 moles

Moles of CCl4 = 50.0 g / 153.82 g.mol-1 = 0.325 moles

Total moles = 0.657 +0.325 = 0.982 moles

So mole fraction of CS2 = 0.657 moles / 0.982 mole = 0.669

Mole fraction of CCl4 = 0.325 moles / 0.982 moles = 0.331

So the partial pressure of CS2 = mole fraction * vapor pressure

                                                = 0.669 * 360 torr

                                                 = 240.8 torr

Partial pressure of CCl4 = 0.331* 99.8 torr

                                     = 33.04 torr

So,total pressure = 240.8 +33.04 = 273.8 torr

                            = 274 torr

So, is the total vapor pressure of a solution containing 50.0g of each compound is B. 274 torr


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