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Question

During which of the following processes, does entropy decrease?


(A) Freezing of water to ice at 0°C

(B) Freezing of water to ice at -10°C

(C) N2(g)+3H2(g)2NH3(g)

(D) Adsorption of CO (g) on lead surface.

(E) Dissolution of NaCl in water

A
(A), (B), (C) and (D) only
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B
(A), (C) and (E) only
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C
(A) and (E) only
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D
(B) and (C) only
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Solution

The correct option is A (A), (B), (C) and (D) only
Answer: (a)

A, B → Freezing of water will decrease entropy as particles will move closer and forces of attraction will increase. This leads to a decrease in randomness. So, entropy decreases.

C → No. of molecules decreasing as we go from reactant to products. So, entropy decreases.

D → Adsorption will lead to a decrease in the randomness of gaseous particles.

ENaCl(s)Na+(aq)+Cl(aq);ΔS>0
Here no of ions increase, so entropy increases.

So, (A, B, C, D) decreases entropy.


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