The salt ammonium sulfate dissolves in water according to the reaction: (NH4)2SO4(s) ------>2NH4+(aq) + SO42-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: ΔH°f(NH4)2SO4(s) = -1180.9 kJ mol-1 ΔH°f NH4+(aq) = -132.5 kJ mol-1 ΔH°f SO42-(aq) = -909.3 kJ mol-1 (b) Calculate the temperature reached by the solution formed when 147 g of (NH4)2SO4 is dissolved in 0.167L of water at 23.1 °C. Approximate the heat capacity of the solution by the heat capacity of 167 g of pure water (specific heat capacity = 4.18 J g-1 °C-1), ignoring the mass of the salt. 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?
The salt ammonium sulfate dissolves in water according to the reaction:
(NH4)2SO4(s) ------>2NH4+(aq) + SO42-(aq)
(a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data:
ΔH°f(NH4)2SO4(s) = -1180.9 kJ mol-1
ΔH°f NH4+(aq) = -132.5 kJ mol-1
ΔH°f SO42-(aq) = -909.3 kJ mol-1
(b) Calculate the temperature reached by the solution formed when 147 g of (NH4)2SO4 is dissolved in 0.167L of water at 23.1 °C. Approximate the heat capacity of the solution by the heat capacity of 167 g of pure water (specific heat capacity = 4.18 J g-1 °C-1), ignoring the mass of the salt.
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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