Problem: 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°C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the specific heat of the resulting solution is 4.18 J/g°C? Is the reaction exothermic or endothermic?

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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°C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the specific heat of the resulting solution is 4.18 J/g°C? Is the reaction exothermic or endothermic?

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Our tutors have indicated that to solve this problem you will need to apply the Constant-Pressure Calorimetry concept. You can view video lessons to learn Constant-Pressure Calorimetry. Or if you need more Constant-Pressure Calorimetry practice, you can also practice Constant-Pressure Calorimetry practice problems.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.