At 63.5 °C, the vapor pressure of H2O is 175 torr, and that of
et...

Question

At 63.5 °C, the vapor pressure of H2O is 175 torr, and that of
ethanol 1C2H5OH2 is 400 torr. (b) Assuming idealsolution behavior, what is the vapor pressure of the solution at 63.5 °C?

Accepted Answer

Hello everyone. Today. We are being given the following question and asked to solve for it. So it says the vapor pressure of benzene is at 20 degrees Celsius as Tour. While that of chloroform is 1 60 Tour, calculate the vapor pressure of the solution prepared by dissolving equal amounts in molds of the two liquids at 20 degrees Celsius. And we are to assume that there is ideal behavior going on. So the first you want to do is you want to find the vapor pressure of a component. And so by doing that we can see the vapor pressure as you go to the P. A. Times the mole fraction times our partial pressures. And so what we have to do is we have to calculate the vapor pressure of benzene in the solution. And since they're made up with equal molar amounts we can go ahead and say that that is going to be equal to 1/ plus one giving us 0.5 for a mole fraction. And so solving for both Benzene and chloroform, We get 0.5 for both mole fractions for the benzene we use 75 tour as indicated in the question and for chloroform we use 160 tour. And when we saw for both of these for Benzene we get 37.5 tour and a detour with chloroform To find the total pressure, we simply have to add these pressures together. And so we take that 37.5 tour and we added to that tour to get a total of 117. tour for our final answer, I hope this helped until next time.

Watch next