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(B) For a chemical reaction to be spontaneous at constant temperature and pressure,the change in Gibbs energy of the system must be negative,i.e.,$\De

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only $(i)$ and $(iv)$

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(B) For a chemical reaction to be spontaneous at constant temperature and pressure,the change in Gibbs energy of the system must be negative,i.e.,$\Delta G_{	ext{sys}} According to the second law of thermodynamics,for any spontaneous process,the total entropy change of the universe (system + surroundings) must be positive,i.e.,$\Delta S_{	ext{total}} = \Delta S_{	ext{sys}} + \Delta S_{	ext{surr}} > 0$. This corresponds to statement $(iv)$.Statement $(ii)$ is incorrect because the total Gibbs energy change for the universe is not a standard criterion for spontaneity.Statement $(iii)$ is not necessarily true because a reaction can be spontaneous even if the entropy change of the system is negative,provided the enthalpy change is sufficiently negative to make $\Delta G$ negative.Therefore,statements $(i)$ and $(iv)$ are always true.

Column $I$	Column $II$
$A$. Freezing of water at $273 \ K$ and $1 \ atm$	$P$. $q=0$
$B$. Expansion of $1 \ mol$ of an ideal gas into a vacuum under isolated conditions	$Q$. $w=0$
$C$. Mixing of equal volumes of two ideal gases at constant temperature and pressure in an isolated container	$R$. $\Delta S_{sys} < 0$
$D$. Reversible heating of $H_{2(g)}$ at $1 \ atm$ from $300 \ K$ to $600 \ K$,followed by reversible cooling to $300 \ K$ at $1 \ atm$	$S$. $\Delta U=0$
	$T$. $\Delta G=0$

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