Problem: HI has a normal boiling point of -35.4°C, and its ΔHvap is 21.16kJ/mol. Calculate the molar entropy of vaporization (ΔSvap).A. 68.6 J/K • molB. 0.068 J/K • molC. 598 J/K • molD. 89.0 J/K • molE. 75.2 J/K • mol

🤓 Based on our data, we think this question is relevant for Professor Paesani's class at UCSD.

Problem Details

HI has a normal boiling point of -35.4°C, and its ΔHvap is 21.16kJ/mol. Calculate the molar entropy of vaporization (ΔSvap).

A. 68.6 J/K • mol
B. 0.068 J/K • mol
C. 598 J/K • mol
D. 89.0 J/K • mol
E. 75.2 J/K • mol

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Entropy concept. You can view video lessons to learn Entropy. Or if you need more Entropy practice, you can also practice Entropy practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofHI has a normal boiling point of -35.4°C, and its ΔHvap is 2...as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Dasha took 2 minutes and 22 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Paesani's class at UCSD.