Assuming that the determined values for delta_dis H^0 and delta_disS^0 are tempe

Question

Assuming that the determined values for delta_dis H^0 and delta_disS^0 are temperature independent, is the dissolution of KNO_3 spontaneous at all temperatures? Justify your answer. Ammonium nitrate(NH_4NO_3) is a highly soluable salt for which the dissolution is endothermic. What can be deduced about delta_disS^0 for this compound? Magnesium sulfate(MgSO_4) is a highly soluable salt for which the solubility decreases with increasing temperature. What can be deduced about delta_disG^0, delta_disH^0, and delta_disS^0 for this compound?

Explanation / Answer

3) Question 3 is blurred unable to clearly read the problem

4) For the reaction to occur, Delta G must be negative

Delta G = Delta H - T * Delta S

Since Delta H is positive (endothermic reaction), hence Delta S must be highly positve in order to make the reaction happen

Delta S >0

5) Since it is highly soluble, it implies that the reaction is favored

Hence Delta G must be negative

Delta H must also ne negative

Since with increase in temperature, the solubility reduces, hence it means Delta S is also negative

Delta G = Delta H - T * Delta S

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