A and B on mixing form an ideal solution at r | vedclass

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(C) For the formation of an ideal solution, the process is spontaneous, which implies $\Delta G < 0$.According to the definition of an ideal solution:

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$\Delta G$$\Delta S_{	ext{system}}$$\Delta S_{	ext{surroundings}}$$\Delta H$$-$$+$$0$$0$

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(C) For the formation of an ideal solution, the process is spontaneous, which implies $\Delta G According to the definition of an ideal solution:$\Delta H_{	ext{mix}} = 0$$\Delta V_{	ext{mix}} = 0$Since $\Delta H_{	ext{mix}} = 0$, there is no heat exchange between the system and the surroundings, so $\Delta S_{	ext{surroundings}} = 0$.Mixing increases the randomness of the components, so $\Delta S_{	ext{system}} > 0$.Using the Gibbs free energy equation: $\Delta G = \Delta H - T\Delta S$.Since $\Delta H = 0$ and $\Delta S > 0$, we get $\Delta G = -T\Delta S$, which is less than $0$ (negative).

$A$ and $B$ on mixing form an ideal solution at room temperature. Which of the following options is correct for this process?

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$\Delta G$	$\Delta S_{\text{system}}$	$\Delta S_{\text{surroundings}}$	$\Delta H$
$-$	$+$	$+$	$+$