It is known that heat energy (enthalpy) is required to separate the associated i

Question

It is known that heat energy (enthalpy) is required to separate the associated ions (bonds) in a solid salt and that heat energy is released when water molecules surround the ions. MgSO4 is one of the best salts as a possible hot pack. However, Epsom salt, MgSO4*7H2O, is used for soaking minor sprains and functions as a cold pack. Based upon the identity of these salts, propose a reason why one can be used as a hot pack and the other as a cold pack. Use the concepts of energy, enthalpy, entropy, endothermic process, and exothermic process in your answer. Do not include lattice energy or hydration energy in the explanation.

Explanation / Answer

exothermic reaction can be used as hot packs.Heat energy is released when water molecules sorround the ions.Magnesium sulfate used as hot pack .In a hot pack there is powdered MgSO4 with a small bag of water.When we squeeze the hot pack the water pack bursts to begin the reaction.magnesium sulfate release energy and water molecules sorround the Mg2+ and SO42- ions.so the reaction is exothermic and we use magnesium sulfate as hot pack.

endothermic reaction can be used as cold packs.Heat energy is required to seprate the associate ions in a solid salts.eposum salt act as cold pack.when the small bag of eposum salt put under pressure it bursts to begin the endothermic reaction .the reaction need energy,so it takes the energy from you,so you will feel cold. Cold is just a sensation of energy moving away from you.

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