Final answer:
The total heat required to change 20.2g of ice to liquid water at 58°C is 11622.432 J, which is calculated by summing the heat of fusion for melting the ice and the heat needed to raise the temperature of the water to the desired temperature.
Step-by-step explanation:
To calculate the heat required to change 20.2g of ice to liquid water at 58°C, we first consider the heat of fusion for ice, which is the energy required to convert ice to water at 0°C. This value is 334 J/g. Then, we must calculate the energy required to raise the temperature of the resulting water from 0°C to 58°C using the specific heat capacity of water, which is 4.184 J/g°C.
The calculation has two steps:
Melting the ice: Heat of fusion × mass = 334 J/g × 20.2 g = 6746.8 JHeating the water: Specific heat capacity × mass × temperature change = 4.184 J/g°C × 20.2 g × 58°C = 4875.632 J
Adding both values together: 6746.8 J + 4875.632 J = 11622.432 J
Therefore, the total heat required is 11622.432 J, which is not listed among the answer choices A to D. So, there might be an error in the question or the answer choices provided.