Published by:
CGP EDU Academic Team
Published on: August 13, 2026
One mole of an ideal diatomic gas (C v = 5 cal) was transformed from initial 25°C and 1 L to the state when temperature is 100°C and volume 10 L. Then for this process(R = 2 calories/mol/K) (take calories as unit of energy and kelvin for temp)
A
Δ H = 525
B
Δ S = 5 ln 
+ 2 ln 10
+ 2 ln 10
C
Δ E = 525
D
Δ G of the process can not be calculated using given information.
Text Solution
Verified by ExpertsThe correct answer is:
CHECK THE SOLUTION.
(a,b,d) Δ S = nC V ln 
+ nR ln 
= 5 ln 
+ 2 ln 10
Δ H = nC P Δ T = n (C V + R) Δ T = 1 × 7 × 75 = 525 cal
Prepare Smarter with CGP Edu
Get practice questions, solutions, and test series in one place.
Write a Review
Share your experience with this question and solution.
Commentary
Send your comment, doubt, correction, or feedback to admin.
Similar Questions
Explore conceptually related problems
Match the column:
Columm-IColumm-II (a)Reversible isothermal expansion of an ideal gas(p)w = –2.303…
Match the column:
Column-IColumn-II(a)A process carried out infinitesimally slowly(p)Adiabatic(b)A …
How many statements are false ?
(i) Thermodynamics is concerned only with total energy of the syste…
How many of the following physical properties are extensive :
(i) Free energy (ii) vapour pressure
…
How many of the following are state function :
(i) Internal energy (ii) Heat
(iii) Enthalpy (iv) En…
Two moles of He gas ( γ = 5/3) are initially at temp 27ºC and occupy a volume of 20 litres. The gas…