Answer :
Final answer:
The final temperature of a mixture of ice and hot water will be between 0°C and 100°C after the ice melts and the remaining heat raises the temperature of the resulting water until equilibrium is reached. The exact temperature requires detailed thermal energy calculations, but is likely closer to the lower end of the range.
Explanation:
The mixture of 100 g of ice at zero degree celsius with 100 g of water at 100 degree celsius involves the transfer of heat between the hot water and the cold ice until thermal equilibrium is reached. As the ice melts, it absorbs heat from the hot water, which cools down in the process. The specific heat of water (4.184 J/g·°C) and the enthalpy of fusion of ice (334 J/g) are critical to calculating the final temperature of the mixture. Since there are equal masses of ice and water, a reference calculation from a closely related problem - where a 50.0 g ice cube at 0.0°C is added to 500 mL of tea at 20.0°C - shows that after the ice cube has melted, the temperature of the tea decreases. Similarly, in our scenario, as the hot water gives off heat, it will convert the ice to liquid water at 0°C. If additional heat is still available after melting the ice, the temperature of the water will start to rise.
However, the exact final temperature can only be determined through detailed calculations involving the conservation of energy principle. We can ascertain that the final temperature will be somewhere between 0°C and 100°C (excluding those temperatures), therefore, options (b) 0 degrees Celsius and (d) 100 degrees Celsius can be eliminated, while option (a) 50 degrees Celsius and (c) 25 degrees Celsius remain as potential answers, potentially leaning towards (c) due to the latent heat absorbed by the melting of ice.
