Question

For a free expansion of an ideal gas in an isolated chamber which of the following statements is true ?
A. Entropy of the system increases
B. Temperature of the system decreases
C. Internal energy of the system decreases
D. Positive work is done by the system

Answer 1

Final Answer :A Entropy of the system increases :

STEPS:
1) Free Expansion :
Irreversible Process in which gas Expands freely in Adiabatic Process.

Now,
A)
=> Since , Gas Expands Freely.
and Change in Entropy is proportional to
$ln( \frac{v(f)}{v(i)} )$
Therefore, Entropy of the system increases.

B) Process is Adiabatic.
So,Niether Heat is released not absorbed.
=> del (Q) = 0
And,
Here, Gas Expands Freely without any External Pressure.
So, Work done by gas = 0
By First Law of Thermodynamic,
del(E) = del(Q) + W
= 0+ 0 =0
So,
Change in Internal Energy =0
=> del( T) = 0
=> T = constant

C) Internal Energy of the system remains constant as del(E) =0
=> E = constant

D) Workdone by the gas is 0 since there is no External Pressure.

Answer 2

Answer:

(A)Entropy of the system increases.

Explanation:

• The measure of disorder present in the system is called entropy.
• It is low for solid state and very high for gaseous substances.

• From the given, for a “free expansion” of an ‘ideal gas’ in an isolated chamber.
• Means gas is transferred from chamber to free expansion.
• It will leads to the increases the irregularity of the molecules than compared to the chamber.

• Hence, the “entropy of the system increases”.