Question

Four blocks of ice (15.0 g each) are added to 200 g of water at 35.0°C. Determine the final temperature of the water.

A) 0.0°C
B) 5.0°C
C) 10.0°C
D) 15.0°C

Answer 1

Heat transfer between the warm water and the ice will result in the ice warming and melting, with the final temperature likely being 0.0°C, assuming that all of the heat from the water is used for these processes.

Step-by-step explanation:

To determine the final temperature of the water after adding four blocks of ice, we must consider the heat transfer between the water and the ice. The heat lost by the water will be used to first warm the ice to 0°C, then melt the ice, and finally, if any heat remains, to warm the water that resulted from the melted ice. The specific heats of liquid water and ice, along with the enthalpy of fusion (heat required to melt ice), are essential here. However, since we are not provided with specific heat values or the enthalpy of fusion for the purpose of solving the problem, and since the problem's statement does not mention reaching a temperature above 0°C, we may infer that all the heat from the warm water goes into melting the ice and possibly warming the ice up to 0°C, suggesting that the final temperature will not exceed 0°C. Considering that, the most likely answer would be 0.0°C, but to provide a certain answer, we would need the aforementioned missing values.