Calculating the Heat Required to Heat Ice from -10°C to 0°C

Understanding the amount of heat required to change the temperature of substances is crucial in physics and engineering applications. In this article, we will delve into the calculation of the heat required to heat 1 kg of ice from -10°C to 0°C. This topic is of significant importance in various fields, including refrigeration, climate science, and thermodynamics.

Introduction to Specific Heat Capacity and Temperature Change

The formula to calculate the heat absorbed when changing the temperature of a substance is given by:

Q mcΔT

Q is the heat absorbed in joules. m is the mass of the substance in kilograms. c is the specific heat capacity of the substance in joules per kilogram per degree Celsius (J/kg·°C). ΔT is the change in temperature in degrees Celsius (°C).

Specific Heat Capacity of Ice

For ice, the specific heat capacity c is approximately 2090 J/kg·°C. This value represents the amount of heat required to raise the temperature of 1 kg of ice by 1 °C.

Calculation Example

Given the following values:

m 1 kg c 2090 J/kg·°C ΔT 0 - (?10) 10 °C

The calculation for the heat required is as follows:

Q m c Δ Q 1 kg × 2090 J/kg·°C × 10 °C

Q 20900 J

Therefore, the amount of heat required to heat 1 kg of ice from -10°C to 0°C is 20,900 joules.

Additional Considerations

It is essential to note that there will be no change in volume or pressure until the phase change at 0°C occurs. The formula for heat required during this temperature change is:

Heat mCT

m mass 1 kg C calorific value of water 4.8 kJ/kg/°C T change in temperature 10 °C

Heat 1 kg × 4.8 kJ/kg/°C × 10 °C 48 kJ

Conclusion

In summary, the heat required to heat 1 kg of ice from -10°C to 0°C can be calculated using the specific heat capacity of ice and the change in temperature. Understanding these principles is vital for various applications and can be further expanded to more complex scenarios involving phase changes.