Final answer:
To calculate the energy required to change 10 grams of ice at -2°C to water at 20°C, we must heat the ice to melting point, melt it, and then heat the water to the final temperature. The total energy required is 4944 J, which isn't one of the options provided.
Step-by-step explanation:
The calculation of the energy required to change 10 grams of ice at -2°C to water at 20°C involves multiple steps that include raising the temperature of ice to its melting point, melting the ice, and then heating the resultant water to the desired temperature.
Step-by-step Calculation:
- Calculate the energy needed to heat the ice from -2°C to 0°C using the specific heat capacity of ice (2.09 J/g°C).
Q1 = m * C_ice * ΔT - Calculate the energy required to melt the ice using the heat of fusion for water (334 J/g).
Q2 = m * L_fusion - Calculate the energy needed to heat the water from 0°C to 20°C using the specific heat capacity of water (4.18 J/g°C).
Q3 = m * C_water * ΔT - Add the three quantities of energy calculated (Q1, Q2, Q3) to find the total energy required.
After calculating the values, the total energy required is found to be Q_total = Q1 + Q2 + Q3 = 768 J + 3340 J + 836 J = 4944 J, which is none of the options given (A) 3840 J, (B) 4186 J, (C) 4260.92 J, and (D) 4676.9 J.