Amongst the chemical reactions given below, t | vedclass

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(C) Entropy $(S)$ increases when the disorder of the system increases, such as phase changes from liquid to gas or an increase in the number of gaseou

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$(i)$, $(ii)$, $(iv)$

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(C) Entropy $(S)$ increases when the disorder of the system increases, such as phase changes from liquid to gas or an increase in the number of gaseous moles.$(i)$ $H_2O_{(l)} ightarrow H_2O_{(g)}$: Phase change from liquid to gas increases entropy.$(ii)$ $C_{(s)} + CO_{2(g)} ightarrow 2CO_{(g)}$: The number of gaseous moles increases from $1$ to $2$, so entropy increases.$(iii)$ $2H_{2(g)} + O_{2(g)} ightarrow 2H_2O_{(l)}$: Gaseous reactants form a liquid product, so entropy decreases.$(iv)$ $N_{2(g)} + O_{2(g)} ightarrow 	ext{Mixture of } N_2 	ext{ and } O_2$: Mixing of gases increases the randomness of the system, so entropy increases.Therefore, reactions $(i)$, $(ii)$, and $(iv)$ show an increase in entropy.

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One mole of an ideal diatomic gas $(C_V = 5 \ cal)$ was transformed from initial $25 \ ^{\circ}C$ and $1 \ L$ to the state when temperature is $100 \ ^{\circ}C$ and volume $10 \ L$. The entropy change of the process can be expressed as $(R = 2 \ cal / mol \cdot K)$ :-

Which of the following statements is correct?

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