How much energy is required to convert 360 gram of ice having temp -10 c to convert in to steam
To find the amount of energy required to convert 360 grams of ice at -10°C to steam, we need to calculate the energy required for each phase change.
Here are the steps to find the answer:
1. Calculate the energy required to raise the temperature of the ice from -10°C to 0°C.
The specific heat capacity of ice is 2.09 J/g°C.
The temperature change is 0°C - (-10°C) = 10°C.
So, the energy required for this step is (360 g) × (10°C) × (2.09 J/g°C).
2. Calculate the energy required to melt the ice to water at 0°C.
The heat of fusion for water is 334 J/g.
The mass of the ice is still 360 g, so the energy required for this step is (360 g) × (334 J/g).
3. Calculate the energy required to raise the temperature of the water from 0°C to 100°C.
The specific heat capacity of water is 4.18 J/g°C.
The temperature change is 100°C - 0°C = 100°C.
So, the energy required for this step is (360 g) × (100°C) × (4.18 J/g°C).
4. Calculate the energy required to convert the water to steam at 100°C.
The heat of vaporization for water is 2257 J/g.
The mass of the water is still 360 g, so the energy required for this step is (360 g) × (2257 J/g).
5. Add up all the energies calculated in the previous steps to get the total energy required.
Let's plug the numbers into the equations:
Energy for temperature change: (360 g) × (10°C) × (2.09 J/g°C) = 7,524 J
Energy for melting: (360 g) × (334 J/g) = 120,240 J
Energy for temperature change: (360 g) × (100°C) × (4.18 J/g°C) = 1,507,200 J
Energy for vaporization: (360 g) × (2257 J/g) = 812,520 J
Total energy required = 7,524 J + 120,240 J + 1,507,200 J + 812,520 J = 2,447,484 J
Therefore, approximately 2,447,484 Joules of energy are required to convert 360 grams of ice at -10°C to steam.