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Chapter 5: Q25E (page 270)

Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter (Figure 5.12) at 22.4掳C causes the temperature to rise to 25.8掳C. What is the approximate amount of heat involved in the dissolution, 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 16176.6 J and it is an exothermic reaction.

Step by step solution

01

Heat involved in the dissolution

Given information:

The mass of the water = 150.0 g

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

Rise in the temperature = 25.8 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,

\({\rm{Q = 150 }} \times {\rm{ 4}}{\rm{.18 }} \times {\rm{ 25}}{\rm{.8 = 16176}}{\rm{.6 J}}\).

02

Exothermic reaction

In exothermic reactions, the heat is evolved which leads to a rise in the temperature.Therefore, in the given reaction, a huge amount of heat is evolving, which is why it will be an exothermic reaction.

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