Final answer:
When 0.02kg of ice and 0.1kg of water at 0⁰C are in a container. The final amount of water in the container is 0 kg as all the water has turned into steam.
Step-by-step explanation:
To determine the final amount of water in the container, we need to consider the changes in heat and phase changes that occur during the process. First, let's calculate the heat required to melt the ice. The heat required can be calculated using the formula:
Q = m * L
Where
Q is the heat, m is the mass
L is the latent heat of fusion for ice.
The latent heat of fusion for ice is 334,000 J/kg.
Given that the mass of ice is 0.02 kg, the heat required to melt the ice is:
Q = 0.02 kg * 334,000 J/kg = 6,680 J
Next, let's calculate the heat gained by the water.
The heat gained can be calculated using the formula:
Q = m * c * ΔT
Where
Q is the heat
m is the mass
c is the specific heat capacity
ΔT is the change in temperature.
The specific heat capacity of water is 4,186 J/kg°C. Given that the mass of water is 0.1 kg and the initial and final temperatures are both 0°C, the heat gained by the water is:
Q = 0.1 kg * 4,186 J/kg°C * 0°C = 0 J
Since the heat gained by the water is 0 J and the heat required to melt the ice is 6,680 J, the final amount of water in the container is 0 kg.
Therefore, all the water has turned into steam.