How Much Ice Was in the Calorimeter Initially?

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To determine the mass of ice initially present in the calorimeter, the heat gained by the ice and water must equal the heat lost by the heated aluminum. The specific heat capacity of aluminum is 0.22 cal/g°C, and the system involves a mixture of water and ice at 0°C, which absorbs heat as it melts and warms. The final temperature of the mixture after the aluminum is added is 5°C, indicating a temperature change that can be calculated using heat transfer equations. Conservation of energy principles apply, meaning the total heat gained by the mixture equals the total heat lost by the aluminum. Proper application of these equations will yield the mass of ice in the initial mixture.
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id appreciate some input u guys...

Heat Transfer and Calorimetry

A 50 g Aluminum calorimeter contains 95 g of a mixture of water and ice at 0 degree Celsius. When 100 g of Aluminum, which has been heated in a steam jacket to 100 degree Celsius, is dropped into the mixture, the temperature rises to 5 degree Celsius. Find the mass of ice originally present in the mixture if the specific heat capacity of aluminum is 0.22 cal/g*C
 
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How about you show your work. If you are completely lost on how to begin this problem, and thus have no work to show, then you should look up the heat/temperature change equations and the heat/phase change equations. Also remember the conservation of energy laws - heat gained equals heat lossed.
 

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