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Chapter 5: Q24E (page 270)

A 0.500-g sample of KCl is added to 50.0 g of water in a calorimeter (Figure 5.12). If the temperature decreases by 1.05掳C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g掳C? Is the reaction exothermic or endothermic?

Short Answer

Expert verified

The heat involved in the dissolution is 221.644 J and it is an endothermic reaction.

Step by step solution

01

Heat involved in the dissolution

Given information:

The mass of the sample = 0.500g

The mass of the water = 50.0g

Thus, the total mass of the calorimeter = 0.50 + 50 = 50.5g

The specific heat of the solution = 4.8 J/g掳C

Rise or change in the temperature = 1.05掳C

The heat evolved during the reaction is mathematically presented as \({\rm{Q = mC}}\Delta {\rm{T}}\). Therefore, by putting all the given values in \({\rm{Q = mC}}\Delta {\rm{T}}\), we get,

\({\rm{Q = 50}}{\rm{.5 }} \times {\rm{ 4}}{\rm{.18 }} \times {\rm{ 1}}{\rm{.05 = 221}}{\rm{.644 J}}\)

02

Endothermic reaction

In endothermic reactions, the heat is absorbed, which leads to a decrease in the temperature.Therefore, in the given reaction, the positive sign of heat signifies that the reaction is endothermic.

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