A community for students.
Here's the question you clicked on:
 0 viewing
adamconner
 2 years ago
for the process of H2O (g) > H2O (l)
a) ΔH is negative and ΔS is negative.
b) ΔH is negative and ΔS is positive.
c) ΔH is positive and ΔS is positive
d) ΔH is positive and ΔS is negative.
adamconner
 2 years ago
for the process of H2O (g) > H2O (l) a) ΔH is negative and ΔS is negative. b) ΔH is negative and ΔS is positive. c) ΔH is positive and ΔS is positive d) ΔH is positive and ΔS is negative.

This Question is Closed

adamconner
 2 years ago
Best ResponseYou've already chosen the best response.0ok, I know the entropy will be negative because you are going from a gas to a liquid, so decreasing entropy. but what about the enthalpy ?

Gebooors
 2 years ago
Best ResponseYou've already chosen the best response.3Because water vapour condenses, it gives away heat, so Process is exothermic. That is way delta H is negative. Because delta S = delta H/ T, it is also negative
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.