The enthalpy of solution of CaCl2 is -82.88kJ. If the specific heat of the solution is 4.184J/g*C and the calorimeter constant can be neglected, what will be the final temperature after 5.36g of CaCl2 is dissolved in 100.0g of H2O at 25.0C?
I assume the enthalpy given is kj/mole.
Mutiply that enthalpy by the fraction of mole (5.36/molmassCaCl2), set it equal to mcDeltaT, and solve for deltaT. Use 100 g as the mass of the water, and c for water.
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Please why are we using just the mass of water and not the total mass of the solution
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