Chloroform has ΔHvaporization = 29.2 kJ>mol and boils at 61.2 °C. What is the value of ΔSvaporization for chloroform?

Video transcript

Hello. This problem we're told the change in entropy of vaporization for octonal is 70.1 killed joules per mole. It has a boiling point of 100 95 degrees Celsius. We asked what is its change in entropy of vaporization? So the change in gibbs free energy is equal to the change in entropy minus temperature times The change in entropy when we have water in equilibrium with its vapor which occurs at the boiling point, then Change in Gibbs free energy is equal to zero and so we can relate then the change in entropy to the change in entropy, remove the entropy term to the right hand side, we'll isolate entropy So we get the change in entropy divided by the temperature. We're told the change in entropy was 70.1 pill jules per mole. The boiling point is 195°C. So we'll convert that to Kelvin and our units for hp are usually in jewels. So we're gonna convert then are killed jules to jules. Our units of kill jules will cancel and so this works out then 250 jewels per kelvin mole. This then corresponds to answer. See thanks for watching. Hope this helped