Problem: Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter (Figure 5.12) at 22.4°C causes the temperature to rise to 25.8°C. What is the approximate amount of heat involved in the dissolution, assuming the specific heat of the resulting solution is 4.18 J/g°C? Is the reaction exothermic or endothermic?

FREE Expert Solution

$\overline{){\mathbf{+}}{{\mathbf{q}}}_{{\mathbf{dissolution}}}{\mathbf{=}}{\mathbf{-}}{{\mathbf{q}}}_{{\mathbf{solution}}}}$

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{mc\Delta T}}}$

$\overline{){{\mathbf{q}}}_{{\mathbf{dissolution}}}{\mathbf{=}}{\mathbf{-}}\mathbf{\left(}{\mathbf{m}}_{\mathbf{solution}}\mathbf{c\Delta T}\mathbf{\right)}}$

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Problem Details

Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter (Figure 5.12) at 22.4°C causes the temperature to rise to 25.8°C. What is the approximate amount of heat involved in the dissolution, assuming the specific heat of the resulting solution is 4.18 J/g°C? Is the reaction exothermic or endothermic?