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The salt cesium perchlorate dissolves in water according to the reaction: CsClO4(s) Cs+(aq) + ClO4-(aq) (a)...

The salt cesium perchlorate dissolves in water according to the reaction: CsClO4(s) Cs+(aq) + ClO4-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data:

CsClO4(s) = -443.1 kJ mol^-1

Cs^+(aq) = -258.3 kJ mol^-1

ClO4-(aq) = -129.3 kJ mol^-1

_____kJ

(b) Calculate the temperature reached by the solution formed when 30.0 g of CsClO4 is dissolved in 0.119 L of water at 23.0 °C. Approximate the heat capacity of the solution by the heat capacity of 119 g of pure water (specific heat capacity = 4.18 J g^-1 °C^-1), ignoring the mass of the salt.

____ °C

(c) Heats of reaction find practical application in hot packs or cold packs. Would this dissolution reaction be appropriate for the preparation of a hot pack* or a cold pack*?

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