Introduction:
To calculate the amount of heat required to evaporate the water formed from 10 gm of ice at 0 degrees Celsius, we need to consider the heat transfer involved in the process. The heat transfer occurs in two steps: first, the ice is heated to its melting point, and secondly, the water is heated to its boiling point and then evaporated.

Step 1: Heating the ice to its melting point:
To heat the ice from 0 degrees Celsius to its melting point, we need to calculate the heat required using the formula:
Q = mcΔT
where Q is the heat required, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.

In this case, the mass of the ice is 10 gm and the specific heat capacity of ice is approximately 2.09 J/g°C. The change in temperature is the difference between the melting point of ice (0 degrees Celsius) and the initial temperature (also 0 degrees Celsius), which is 0°C.

Using the formula, we can calculate the heat required to heat the ice to its melting point:
Q1 = (10 gm) * (2.09 J/g°C) * (0°C - 0°C) = 0 J

Therefore, no heat is required to heat the ice from 0 degrees Celsius to its melting point since the temperature remains constant during this phase change.

Step 2: Heating the water to its boiling point and evaporating:
To heat the water to its boiling point and evaporate it, we need to calculate the heat required using the formula:
Q = mcΔT
where Q is the heat required, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.

In this case, the mass of the water formed is also 10 gm (since the ice and water have the same mass) and the specific heat capacity of water is approximately 4.18 J/g°C. The change in temperature is the difference between the boiling point of water (100 degrees Celsius) and the initial temperature (0 degrees Celsius), which is 100°C.

Using the formula, we can calculate the heat required to heat the water to its boiling point and evaporate it:
Q2 = (10 gm) * (4.18 J/g°C) * (100°C - 0°C) = 4180 J

Therefore, the amount of heat required to evaporate the water formed from 10 gm of ice at 0 degrees Celsius is 4180 J.

Conclusion:
To evaporate the water formed from 10 gm of ice at 0 degrees Celsius, a total of 4180 J of heat needs to be supplied to the apparatus. This heat is required to heat the water to its boiling point and then provide the energy necessary for the phase change from liquid to gas.