An isolated box is divided into two equal compartments by a partition (see figure). One compartment contains a van der Waals gas while the other compartment is empty. The partition between the two compartments is now removed. After the gas has filled the entire box and equilibrium has been achieved, which of the following statement(s) is(are) correct?a)Internal energy of the gas has not changed.b)Internal energy of the gas has decreased.c)Temperature of the gas has increased.d)Temperature of the gas has decreased.Correct answer is option 'A,D'. Can you explain this answer?

Question

Answer

Here in the question already specified that equilibrium has achieved after removing the partition,Hence the compartment should have vanderwaal gas thereby internal energy remain as same
for Vander Waal Gas, dU=CvT-a/CdV
(before partion) ∆

After partion dU=cvdT+a/V²dV
Here dV (total volume) changes hence Temperature dT must decrease because V inversely proportional to T in ideal vanderwaal gas equation

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