How much energy is released when 10 gm of steam at 100 degree Celsius turns to ice at 0 degree Celsius

To calculate the energy released when steam at 100 degrees Celsius turns into ice at 0 degrees Celsius, we need to consider two processes: the cooling of the steam from 100 degrees Celsius to 0 degrees Celsius and the condensation of the steam into liquid water and subsequent freezing to form ice.

1. Cooling of the steam:
The amount of energy released when cooling a substance can be determined using the specific heat capacity formula:

Q = m * c * ΔT

where:
Q = energy released
m = mass of the substance
c = specific heat capacity of the substance
ΔT = change in temperature

For water, the specific heat capacity is approximately 4.18 joules/gram·degree Celsius. So, let's calculate the energy released during the cooling of steam:

Q1 = m * c * ΔT1

m = 10 g (given)
c = 4.18 J/g·°C (specific heat capacity of water)
ΔT1 = 100°C - 0°C = 100°C

Q1 = 10 g * 4.18 J/g·°C * 100°C
Q1 = 4180 J

Therefore, during the cooling process, 4180 Joules of energy is released.

2. Condensation and freezing of steam into ice:
The energy released during the phase change from steam to water (condensation) and then from water to ice (freezing) can be calculated using the specific heat of fusion and vaporization for water.

The specific heat of fusion (heat required to convert water into ice at the melting point) is approximately 334 J/g, and the specific heat of vaporization (heat required to convert water into steam at boiling point) is approximately 2260 J/g.

Let's calculate the energy released during the phase changes:

Q2 = m * heat of vaporization + m * heat of fusion

m = 10 g (given)

Q2 = 10 g * (334 J/g + 2260 J/g)
Q2 = 10 g * 2594 J/g
Q2 = 25940 J

Therefore, during the condensation and freezing process, an additional 25940 Joules of energy is released.

Adding up both values, the total energy released is:

Total energy released = Q1 + Q2
Total energy released = 4180 J + 25940 J
Total energy released = 30120 J

Hence, approximately 30120 Joules of energy is released when 10 grams of steam at 100 degrees Celsius turns into ice at 0 degrees Celsius.

To calculate the amount of energy released when 10 grams of steam at 100 degrees Celsius turns into ice at 0 degrees Celsius, we need to consider two processes: the cooling of the steam from 100 degrees Celsius to 0 degrees Celsius, and the phase change from steam to ice.

1. Cooling of steam from 100 degrees Celsius to 0 degrees Celsius:
The specific heat capacity of water is 4.18 J/g·°C (Joules per gram per degree Celsius). We can use this value to determine the energy needed to cool the steam to 0 degrees Celsius.

Energy = mass × specific heat capacity × temperature change

Energy = 10 g × 4.18 J/g·°C × (0°C - 100°C)
Energy = 10 g × 4.18 J/g·°C × -100°C
Energy = -41,800 J

The negative sign indicates that energy is being released during cooling.

2. Phase change from steam to ice:
The heat of fusion for water is 334 J/g. This is the amount of energy required to change the phase from steam to ice at 0 degrees Celsius.

Energy = mass × heat of fusion

Energy = 10 g × 334 J/g
Energy = 3340 J

The total energy released is the sum of the energy released during cooling and the energy released during the phase change.

Total energy released = Cooling energy + Phase change energy
Total energy released = -41,800 J + 3,340 J
Total energy released = -38,460 J

The total energy released when 10 grams of steam at 100 degrees Celsius turns into ice at 0 degrees Celsius is approximately -38,460 Joules.