Final answer:
The heat gained by the cold water (Q1) is calculated using the mass of the cold water and the temperature change to the final temperature. The heat gained by the calorimeter and stirrer (Q2) is calculated using the mass of the hot water that cooled down and its temperature change.
Step-by-step explanation:
The question involves calculating the heat gained by the cold water and the heat gained by the calorimeter and stirrer during a mixing process in a calorimetry experiment. According to the given information, we use the formula Q = m × C × ΔT, where Q is the heat gained or lost, m is the mass, C is the specific heat capacity of water (4.18 J/g°C), and ΔT is the change in temperature.
To find the heat gained by the cold water (Q1), we use the mass of cold water (m1 = 358.98 g) and the temperature change from its initial temperature to the final temperature: Q1 = 358.98 g × 4.18 J/g°C × (51.0°C - 24.0°C).
The heat gained by the calorimeter and stirrer (Q2) can be approximated by assuming that the calorimeter has a negligible heat capacity compared to the mass of water, thus the calculation only considers the heat gain by the mass of the hot water that cooled down: Q2 = 189.47 g × 4.18 J/g°C × (97.0°C - 51.0°C). It is important to note that in a real experiment we also need to consider the specific heat capacity of the calorimeter, but it is not provided in this question.