(C) For reaction $(I)$:$2 Cl_{(g)} \longrightarrow Cl_{2(g)}$$\Delta n_g = 1 - 2 = -1$Since the number of moles of gas decreases,the entropy decreases

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(C) For reaction $(I)$:$2 Cl_{(g)} \longrightarrow Cl_{2(g)}$$\Delta n_g = 1 - 2 = -1$Since the number of moles of gas decreases,the entropy decreases,so $\Delta S For reaction $(II)$:$CO_{2(g)} \longrightarrow CO_{(g)} + \frac{1}{2} O_{2(g)}$$\Delta n_g = (1 + 0.5) - 1 = 0.5$Since the number of moles of gas increases,the entropy increases,so $\Delta S > 0$.Therefore,the signs are negative and positive.

Class 11 Chemistry Thermodynamics 2 nd Law of thermodynamics and Entropy

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For the reactions,
$2 Cl_{(g)} \longrightarrow Cl_{2(g)}$
$CO_{2(g)} \longrightarrow CO_{(g)} + \frac{1}{2} O_{2(g)}$
What are the signs of $\Delta S$,respectively?

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A
Positive and positive
B
Positive and negative
C
Negative and positive
D
Negative and negative

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For the reactions,$2 Cl_{(g)} \longrightarrow Cl_{2(g)}$$CO_{2(g)} \longrightarrow CO_{(g)} + \frac{1}{2} O_{2(g)}$What are the signs of $\Delta S$,respectively?

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For a reversible expansion of $5 \, \text{mol}$ of an ideal gas at $27 \, ^\circ\text{C}$ from a volume of $8 \, \text{dm}^3$ to $80 \, \text{dm}^3$,the change in entropy is ...... $J \, K^{-1}$.

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For the reactions,
$2 Cl_{(g)} \longrightarrow Cl_{2(g)}$
$CO_{2(g)} \longrightarrow CO_{(g)} + \frac{1}{2} O_{2(g)}$
What are the signs of $\Delta S$,respectively?

Observe the following reactions:
$I$. $CaCO_{3(s)} \rightarrow CaO_{(s)} + CO_{2(g)}$
$II$. $Cl_{2(g)} \rightarrow 2 Cl_{(g)}$
$III$. $H_2O_{(l)} \rightarrow H_2O_{(s)}$
Identify the reactions in which entropy increases.