LIVE Course for free

Rated by 1 million+ students
Get app now
JEE MAIN 2023
JEE MAIN 2023 TEST SERIES
NEET 2023 TEST SERIES
NEET 2023
CLASS 12 FOUNDATION COURSE
CLASS 10 FOUNDATION COURSE
CLASS 9 FOUNDATION COURSE
CLASS 8 FOUNDATION COURSE
0 votes
46 views
in Chemistry by (74.5k points)
closed by
Calculate the entropy change when `3.6g` of liquid water is completely converted into vapour at `100^(@)C` . The molar heat of vaporization is `40.85KJ mol^(-1)` .
A. `6.08 JK^(-1)`
B. `109.5JK^(-1)`
C. `21.89JK^(-1)`
D. `-21.89JK^(-1)`

1 Answer

0 votes
by (74.1k points)
selected by
 
Best answer
Correct Answer - 3
`DeltaW_(vap)=40850J mol^(-1),T_(b)=373K`
`DeltaS_(vap)=(DeltaH_(vap))/(T_(b))=(40850J mol^(-1))/(373K)=109.5K^(-1)mol^(-1)`
`DeltaS_(vap)` per gram`=(505.5JK^(-1)mol^(-1))/(18gmol^(-1))=6.083JK^(-1)g^(-1)`
Entropy change for `3.6g` water `=6.083JK^(-1)g^(-1)xx3.5g=21.69JK^(-1)`

Welcome to Sarthaks eConnect: A unique platform where students can interact with teachers/experts/students to get solutions to their queries. Students (upto class 10+2) preparing for All Government Exams, CBSE Board Exam, ICSE Board Exam, State Board Exam, JEE (Mains+Advance) and NEET can ask questions from any subject and get quick answers by subject teachers/ experts/mentors/students.

Categories

...