A) \[21\,(g)\xrightarrow{{}}{{I}_{2}}(g)\]
B) \[CaC{{O}_{3}}(s)\xrightarrow{\Delta }CaO(s)+C{{O}_{2}}(g)\]
C) \[{{H}_{2}}O(l)\xrightarrow{{}}{{H}_{2}}O(s)\]
D) \[N{{a}^{+}}(g)+C{{l}^{-}}(g)\xrightarrow{{}}NaCl(s)\]
Correct Answer: B
Solution :
The solid \[CaC{{O}_{3}}(s)\] with low entropy is transformed into a solid\[CaO(s)\] with low entropy. and a gas \[C{{O}_{2}}\] with high entropy. Hence, \[\Delta S\], entropy change is positive.
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