Answer :
The final temperature of the mixture will be 100°C, which is the boiling point of water while the mass of ice (m_ice) will be 0 g.
How to get the Final Temperature?
To determine the final temperature of the tea and the mass of ice, we can use the principle of conservation of energy and the heat equation. When the hot water and ice mix, heat will be transferred from the hot water to the ice until they reach thermal equilibrium.
The equation for heat transfer is:
Q = m * c * ΔT
Where:
- Q is the heat transferred
- m is the mass of the substance
- c is the specific heat capacity of the substance
- ΔT is the change in temperature
Assuming no heat is lost to the surroundings and the final temperature is the same for both substances, we can set up the equation:
Q_hot water = Q_ice
m_hot water * c_hot water * ΔT_hot water = m_ice * c_ice * ΔT_ice
Since the ice is initially at 0°C and we're assuming the hot water is significantly hotter than that, the equation simplifies to:
m_hot water * c_hot water * ΔT_hot water = m_ice * c_ice * 0
Given that the mass of hot water (m_hot water) is 520 g and the specific heat capacity of water (c_hot water) is about 4.18 J/g°C, and the specific heat capacity of ice (c_ice) is about 2.09 J/g°C, we can solve for the mass of ice (m_ice):
520 g * 4.18 J/g°C * ΔT_hot water = m_ice * 2.09 J/g°C * 0
ΔT_hot water = final temperature - initial temperature
ΔT_hot water = final temperature - 100°C (assuming the hot water was initially boiling)
Now, solving for m_ice:
520 g * 4.18 J/g°C * (final temperature - 100°C) = 0
Solving for the final temperature:
final temperature - 100°C = 0
final temperature = 100°C
The final temperature of the mixture will be 100°C, which is the boiling point of water.
As for the mass of ice (m_ice), it will be 0 g. This means that all the ice has melted and reached the same temperature as the hot water, resulting in a mixture of only liquid water at 100°C.
Learn more about conservation of energy here: https://brainly.com/question/27422874
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