Calculate Heat Required for Phase Transition from Ice to Water
How much heat is required to convert 6.13 g of ice at -13.0°C to water at 30.0°C?
What are the steps involved in calculating the heat needed for this phase transition?
Answer:
The heat required to convert 6.13 g of ice at -13.0°C to water at 30.0°C involves three main steps:
- Heating the ice from -13.0°C to 0°C
- Melting the ice at 0°C
- Heating the resulting water from 0°C to 30.0°C
Calculating the heat required for this phase transition involves specific heat capacities and the latent heat of fusion. The specific heat capacity of ice (c_ice) is 2.09 J/g°C, the latent heat of fusion for water (L_f) is 334 J/g, and the specific heat capacity of water (c_water) is 4.18 J/g°C.
To find the heat needed for each step, we use the formulas:
Heating ice from -13.0°C to 0°C: Q1 = m * c_ice * ΔT
Melting ice at 0°C: Q2 = m * L_f
Heating water from 0°C to 30.0°C: Q3 = m * c_water * ΔT
By adding up the heat calculated from each step, we can determine the total amount of heat required for the phase transition from ice to water. This process involves considering the specific heat capacities and the latent heat of fusion to accurately calculate the amount of heat needed.