Suppose you have an ice cube that has a mass of 11.58g at a temperature of -2.8°C. If you add this ice to 71.49g of insulated water at a temperature of 59°C, what is the final temperature of the mixture in °C?
Suppose you have an ice cube that has a mass of 11.58g at a temperature of -2.8°C. If you add this ice to 71.49g of insulated water at a temperature of 59°C, what is the final temperature of the mixture in °C?
Absorbing the heat from the hot water, the temperature of the ice will first increase to , then it will change its state from solid to liquid and then again the temperature of the icy water will increase to the final equilibrium temperature. On the other hand, the hot water release the heat to reach to the final equilibrium temperature.
The amount of heat absorbed by the ice to change its temperature form to can be written as
Here, is the absorbed heat to change the temperature, is the mass, is the specific heat, is the melting point and is the initial temperature of the ice.
The amount of heat absorbed by the ice to change its state from solid to liquid can be written as
Here, is the heat absorbed by the ice to change its state and is the latent heat of fusion.
The amount of heat absorbed by the ice to reach the equilibrium temperature can be written as
Here, is the heat absorbed by the icy water at freezing point to reach the equilibrium temperature, is the specific heat of water and is the equilibrium temperature.
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