500 grams of water at 0 degrees C was heated to a boiling in a large pot. how much energy was needed? what was the temperature change and Heat energy
heat needed was q = mass water x specific heat water x (100-0) = ??
delta T = 100 C.
To calculate the amount of energy needed to heat water from 0 degrees Celsius to its boiling point, you can use the specific heat capacity formula and the heat of vaporization. Here's how you can calculate it step by step:
1. Calculate the energy required to raise the temperature of water from 0°C to 100°C:
- The specific heat capacity of water is approximately 4.18 Joules/gram°C.
- The temperature change is 100°C (the boiling point) - 0°C (initial temperature).
- Therefore, the energy required for this temperature change is:
Energy = mass × specific heat capacity × temperature change
Energy = 500 g × 4.18 J/g°C × 100°C
2. Calculate the energy required to change the water from liquid to gas (vaporization):
- The heat of vaporization for water is approximately 2260 Joules/gram.
- The mass of the water remains the same during a phase change.
- Therefore, the energy required for vaporization is:
Energy = mass × heat of vaporization
Energy = 500 g × 2260 J/g
To find the total energy required, add up the energy for temperature change and vaporization:
Total Energy = Energy for temperature change + Energy for vaporization
You can now substitute the values into the equations to get the final answer.