Dear beloved readers, welcome to our website! We hope your visit here brings you valuable insights and meaningful inspiration. Thank you for taking the time to stop by and explore the content we've prepared for you.
------------------------------------------------ a solution is composed of 1.30 moles of a and 2.00 moles of b, both volatile components . what is the total vapor pressure above this solution? the vapor pressure of pure a is 97.6 torr and the vapor pressure of pure b is 229.5 torr at this temperature. total vapor pressure

To determine the total vapor pressure above the solution, we can use Raoult's Law, which states that the vapor pressure of a component in a solution is directly proportional to its mole fraction in the solution.

Let's calculate the mole fraction of each component first:

Mole fraction of A (Xa) = moles of A / total moles of solution

= 1.30 moles / (1.30 moles + 2.00 moles)

= 0.393

Mole fraction of B (Xb) = moles of B / total moles of solution

= 2.00 moles / (1.30 moles + 2.00 moles)

= 0.607

Now, we can calculate the partial pressure of each component:

Partial pressure of A (Pa) = Xa * vapor pressure of A

= 0.393 * 97.6 torr

= 38.33 torr

Partial pressure of B (Pb) = Xb * vapor pressure of B

= 0.607 * 229.5 torr

= 139.32 torr

Finally, the total vapor pressure above the solution is the sum of the partial pressures:

Total vapor pressure = Pa + Pb

= 38.33 torr + 139.32 torr

= 177.65 torr

Therefore, the total vapor pressure above this solution is approximately 177.65 torr.

learn more about Raoult's Law here:

https://brainly.com/question/2253962

#SPJ11