When 0.250 moles of KCl are added to 200.0 g of water in a constant pressure calorimeter a temperature change is observed. Given that the specific heat of the resulting solution is 4.184 J g⁻¹ °C, the molar heat of solution of KCl is +17.24 kJ/mol, and that we can ignore the small amount of energy absorbed by the calorimeter, the observed temperature change should be ________.Hint: Make sure you convert to moles within the problem.

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The Answer of When 0.250 moles of KCl are added to 200.0 g of water in a constant pressure calorimeter a temperature change is observed. Given that the specific heat of the resulting solution is 4.184 J g⁻¹ °C, the molar heat of solution of KCl is +17.24 kJ/mol, and that we can ignore the small amount of energy absorbed by the calorimeter, the observed temperature change should be ________.Hint: Make sure you convert to moles within the problem.

When 0250 Moles of KCl Are Added to 200