How many joules of heat is required to change 40.0g of ice at 0degrees Celsius to liquid water at 0 degrees Celsius.
q = mass ice x heat fusion
To determine the amount of heat required to change ice to liquid water at the same temperature, several steps need to be considered. Here's a breakdown of the process:
1. Calculate the heat required to heat the ice from -273.15°C (absolute zero) to 0°C.
- The specific heat capacity of ice is 2.09 J/g°C.
- The temperature change is 0°C - (-273.15°C) = 273.15°C.
- Using the formula: Heat = mass * specific heat capacity * temperature change
Heat = 40.0 g * 2.09 J/g°C * 273.15°C.
2. Calculate the heat required to change the ice at 0°C to liquid water at 0°C.
- The heat of fusion (enthalpy of fusion) for water is 334 J/g.
- Using the formula: Heat = mass * enthalpy of fusion
Heat = 40.0 g * 334 J/g.
3. Add up the two calculated heats to find the total heat required.
Total Heat = Heat for heating + Heat for phase change.
Therefore, you can proceed with the calculations:
- Heat for heating = 40.0 g * 2.09 J/g°C * 273.15°C.
- Heat for phase change = 40.0 g * 334 J/g.
Finally, you find the total heat required to change 40.0g of ice at 0°C to liquid water at 0°C by adding the two calculated heats.