Final answer:
To determine the energy required to heat 20.0g of ice from -10.0°C to 45.0°C, it's necessary to calculate the energy for warming the ice up to 0°C, the latent heat to melt the ice, and the energy to increase the temperature of water to 45.0°C. Specific heat capacities and the heat of fusion are used in these calculations.
Step-by-step explanation:
To calculate the amount of energy necessary to convert 20.0g of ice from -10.0°C to 45.0°C, we need to account for the energy required to heat the ice to 0°C, the latent heat of fusion to melt the ice into water, and then the energy needed to raise the temperature of the resulting water to 45.0°C.
Here is the step by step calculation:
- Heat the ice from -10.0°C to 0°C: q = m * Cice * ΔT
- Melt the ice at 0°C: q = m * Lf
- Heat the water from 0°C to 45.0°C: q = m * Cwater * ΔT
Where m is the mass, C is the specific heat capacity, ΔT is the change in temperature, and Lf is the heat of fusion. The specific heat capacity of ice (Cice) is approximately 2.09 J/g°C, the heat of fusion for water (Lf) is 334 J/g, and the specific heat capacity of water (Cwater) is 4.18 J/g°C.
The exact values would need to be inserted along with the mass of the ice to find the total energy required, which would be the sum of all three steps.