Final answer:
The heat transfer for the system, where a 32.9 g iron rod at 22.7 °C is submerged in water at 63.3 °C and the system reaches equilibrium at 59.1 °C, is ΔH = -95.7 kJ, as this represents the total heat change of the system.
Step-by-step explanation:
To calculate the heat transfer for the system, we can use the concept of conservation of energy, where the heat lost by the iron rod will be equal to the heat gained by the water until thermal equilibrium is reached. The final temperature of the system is 59.1 °C. The iron rod's initial temperature is 22.7 °C and its mass is 32.9 g. Since ΔH is given as -95.7 kJ, which is the heat change of the entire system, one would assume that this is the heat change required to bring the entire system to the final temperature. However, without knowing the specific heats or the mass of the water, we cannot determine the exact heat transfer for each component separately. Therefore, based on the provided information, the heat transfer for the system is -95.7 kJ since ΔH represents the heat exchange for the entire system reaching equilibrium.