🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →
Log in
Chemistry
1
answer
0
watching
156
views

(a) Does the entropy of the surroundings increase for spontaneous processes? (b) In a particular spontaneous process the entropy of the system decreases. What can you conclude about the sign and magnitude of ∆Ssurr? (c) During a certain reversible process, the surroundings undergo an entropy change, ∆Ssurr = –78 J/K. What is the entropy change of the system for this process?

Watch
1
answer
0
watching
156
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Casey Durgan
Casey DurganLv2
28 May 2020

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

A Cu wire of diameter of 2 mm and length of 1 m initially at room temperature of 300 K is applied a constant voltage difference of 100 V for 1000 seconds. The temperature of the wire rose due to Joule heating during the application of the voltage, so one waited for a sufficiently long time after the voltage is removed for the wire to cool back to the room temperature of 300 K. The conductivity of Cu is 6×107S/m. Please answer the following questions, assuming the surroundings is at room temperature 300 K:
(a) What is the internal energy change for the wire from the very initial state to the final state after the entire process ends?
(b) What is the internal energy change for the surroundings for the entire process?
(c) What is the amount of heat that was generated in the wire and transferred to the surroundings during the entire process?
(d) What is the total internal energy change of the wire plus the surroundings during the entire process?
(e) What is the entropy change for the wire for the entire process:
(f) What is the entropy change for the surroundings for the entire process?
(g) What is the total entropy generated in the wire and transferred to the surroundings during the entire process?
(h) What is the total entropy change of the wire plus the surroundings during the entire process?
(i) Is this entire process reversible or irreversible?

Can anyone please explain why ∆S(surroundings) is < 0 ???

What do they mean ∆H (system) > 0? How/why did the system provide heat to dissolve the barium sulfate???

What equation are they drawing from? The only equation I can think of to relate this situation is ∆S(universe) = ∆S(system) + ∆S(surroundings) > 0 (if the process is spontaneous).Does it mean it's not spontaneous if the system provided heat? Maybe this has to do with lattices and hydration - I don't know.

apparently, ∆G for the dissolution of barium sulfate in water is positive.. is dissolution of a sparingly soluble salt always a non-spontaneous process? Thank you!

Please help me - thanks!

A well-insulated piston-cylinder assembly containing 5 kg ofwater vapor,
initially at 540 C and 60 bar, undergoes a reversible expansion to20 bar. The surroundings are at 1 bar and 25 C

(a) What is the entropy change of the system, surroundings, anduniverse for this process?
(b) What is the final temperature of water?
(c) What is the work interaction for this process?
(d) What is the final volume of the system?

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in