During which of the following processes, does entropy decrease?
(A) Freezing of water to ice at 0$^\circ$C
(B) Freezing of water to ice at $-$10$^\circ$C
(C) N2(g) + 3H2(g) $\to$ 2NH3(g)
(D) Adsorption of CO(g) on lead surface.
(E) Dissolution of NaCl in water
Choose the correct answer from the options given below :
Solution
A, B $\to$ Freezing of water will decrease entropy as particles will move closer and forces of
attraction will increase. This leads to decrease in randomness. So entropy decrease.<br><br>
C $\to$ No. of molecules decreasing<br><br>
D $\to$ Adsorption will lead to decrease in randomness of gaseous particles.<br><br>
E $\to$ NaCl(s) $\to$ Na<sup>+</sup>(aq) + Cl<sup>–</sup>(aq) $\Delta$S > 0<br><br>
So, (A, B, C, D) decreases entropy.
About this question
Subject: Chemistry · Chapter: Thermodynamics · Topic: Zeroth and First Law
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