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Consider the reaction for the dissolutio...

Consider the reaction for the dissolution of ammonium nitrate:
`NH_(4)NO_(3)(s) rarr NH_(4)^(o+)(aq) +NO_(3)^(Theta) (aq)`
`DeltaH =+29.8 KJ mol^(-1), DeltaS = 108.0 J K^(-1) mol^(-1)`.
Calculate the change in entropy of the surroundings and predict whether the reaction is spontaneous or not at `25^(@)C`?

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To solve the problem, we need to calculate the change in entropy of the surroundings and then determine whether the reaction is spontaneous at 25°C. ### Step 1: Calculate the change in entropy of the surroundings (ΔS_surroundings) The formula for the change in entropy of the surroundings is given by: \[ \Delta S_{\text{surroundings}} = -\frac{\Delta H}{T} ...
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