An ammonium nitrate product dissolves easily in water at room temperature, and the process causes the solution to become quite cold. Which of the following are true about the dissolution of ammonium nitrate?
$I$ . The process is endothermic.
$I I$ . The solubility will be greater in warmer water.
$I I I$ . $S^{o}$ for the reaction is negative.

I

only

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I I

only

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I

and

I I

only

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I

and

I I I

only

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I, I I

and

I I I

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Solution

The correct option is A $I$ only
If dissolution of ammonium nitrate in water decrese the temperature of water, that means, heat is absorbed by the system and the process is endothermic. and on increasing the temperature of water, the solubility of ammonium nitrate will decrease because thr equilibrium will shift in backward direction. and negative value of $S^{0}$ shows the non-spontanity of the reaction.

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