JEE MAIN - Chemistry (2021 - 17th March Evening Shift - No. 7)
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 :
(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 :
(A), (C) and (E) only
(B) and (C) only
(A), (B), (C) and (D) only
(A) and (E) only
Explanation
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.
C $$ \to $$ No. of molecules decreasing
D $$ \to $$ Adsorption will lead to decrease in randomness of gaseous particles.
E $$ \to $$ NaCl(s) $$ \to $$ Na+(aq) + Clā(aq) $$\Delta $$S > 0
So, (A, B, C, D) decreases entropy.
C $$ \to $$ No. of molecules decreasing
D $$ \to $$ Adsorption will lead to decrease in randomness of gaseous particles.
E $$ \to $$ NaCl(s) $$ \to $$ Na+(aq) + Clā(aq) $$\Delta $$S > 0
So, (A, B, C, D) decreases entropy.
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