Given the data in Problem 18.78, calculate ∆G for the vaporization of benzene at: (a) 70 °C Predict whether benzene will boil at each of these temperatures and 1 atm pressure.

Video transcript

Hello everyone today. We have the following problem determine the Gibbs free energy for the vaporization of acetone at 40°C will ask it to a boil at the given temperature and one atmosphere use the following data. So the first thing you do is you want to recall the equation for gibbs free energy that states of the gibbs, free energy is equal to the change in entropy minus temperature times the change in entropy. So we're gonna plug in our values that we have here For our change in entropy we have 29 points 10 kg joules per mole. We're gonna need this answer in terms of jewels so we're gonna have to use the conversion factor that one killer jewels equal to 10 to the third jewels. Killing is canceled out there, We're going to subtract by the temperature that we have which is 40°C. However, this must be in terms of Kelvin. So what we're going to do We're gonna add it to 73. Kelvin And last they were gonna multiply by the change in entropy which is 88.3 jewels. Primal kelvin. After we do our calculations, we're going to get 1448. jewels. However this is not going to be our final answer. We're going to need to convert this back into jewels. So what we're gonna do is we're gonna take our 1448.855 jewels and multiplied by the conversion factor that one killer jewel is equal to 10 to the third jewels. And when our units cancel, we're left with 1.45 killer jewels. So this is the first part of our question here. So we need to find out if it will boil over so it will not actually boil. And so why is this? This is because the gibbs, free energy is not strong enough to overcome the forces needed for a substance to boil, so just in short it won't boil. And with that we have solved the problem overall, I hope this helped and until next time.