How to determine the amount of energy released when 50g of 100C steam changes to 0C ice?
To determine the amount of energy released when steam changes to ice, you need to consider the heat involved in both the phase change (from steam to water) and the temperature change (from water to ice).
To calculate the energy released during the phase change, you can use the equation:
Q = m * L
Where:
Q is the energy released or absorbed
m is the mass of the substance undergoing the phase change
L is the specific latent heat of the substance
For water, the specific latent heat of vaporization (the amount of energy required to change water from a liquid to a gas at constant temperature) is approximately 2260 J/g.
Thus, to calculate the energy released during the phase change from steam to water:
Q1 = m1 * L1
Q1 = 50 g * 2260 J/g
Q1 = 113,000 J
Next, to calculate the energy released during the temperature change from water at 100°C to ice at 0°C, you can use the equation:
Q2 = m2 * C * ΔT
Where:
Q2 is the energy released or absorbed
m2 is the mass of the substance undergoing the temperature change
C is the specific heat capacity of the substance
ΔT is the change in temperature
For water, the specific heat capacity is approximately 4.18 J/g°C.
Thus, to calculate the energy released during the temperature change from water to ice:
Q2 = m2 * C * ΔT
Q2 = 50 g * 4.18 J/g°C * (100°C - 0°C)
Q2 = 209,000 J
Finally, to determine the total energy released when 50g of 100°C steam changes to 0°C ice, you can add the two energy values:
Total energy released = Q1 + Q2
Total energy released = 113,000 J + 209,000 J
Total energy released = 322,000 J