Final answer:
In calorimetry, when CaCl2 is dissolved in water, heat is absorbed by water, resulting in temperature increase. The amount of heat transfer depends on mass, specific heat, and temperature change. For bottles of water, the larger volume lost more heat, and heat measured or absorbed changes based on the calorimeter's insulation efficiency and heat capacity.
Step-by-step explanation:
When 5.00 g of CaCl₂ is dissolved in 50.0 g of water at 23°C within a coffee cup calorimeter, the temperature increase to 39.2°C indicates that heat is absorbed by the water. This process involves an exothermic dissolution reaction where heat is released from the solute (CaCl₂) and absorbed by the solvent (water), raising the temperature. To calculate the amount of heat transferred, we would use the formula: q = m⋅c⋅ΔT, where q represents the heat absorbed or released, m is the mass of the water, c is the specific heat capacity of water (4.18 J/g°C), and ΔT is the change in temperature.
Concerning the calorimetry scenarios with bottles of water: the correct answer is that the 2-L bottle of water lost more heat, as it had a greater mass and therefore required more heat to be removed in order to cool to the same temperature. Errors in the other answers stem from misconceptions about heat transfer and the relationship between mass, temperature change, and heat capacity.
For mixing water to achieve a specific temperature, the Principle of the Conservation of Energy is applied; the heat lost by the hot liquid equals the heat gained by the cooler liquid. In the spoon and coffee mixing problem, the heat transfer between the silver spoon and coffee will cause a mutual temperature that depends on the masses and specific heat capacities of both substances.