An aluminum calorimeter with mass 85g and containing 310g of water are initially at thermal equilibrium at 20 ̊C (room temperature). An ice cube is taken from the freezer with T = –8.5 ̊C and placed in the calorimeter water. When all the ice is melted, the final temperature is 17 ̊C. The specific heat of Al is 900 J/kg ̊C, the specific heat of ice is 2100 J/kg ̊C, and of liquid water is 4186 J/kg ̊C. The latent heat of fusion of water is 3.3x105 J/kg. What was the original mass of the ice cube? You can calculate the original mass of the ice cube in several steps: a) First calculate the total heat lost by the 85g calorimeter and the 310g of liquid water when they are cooled to 17 degrees C. b) To calculate the ice mass, assume all the heat lost by the calorimeter and water from part (a) goes into heating the ice to 0 ̊C, melting the ice at 0 ̊C, and then raising the melted ice (now water) to +17 ̊C, in three steps. The only unknown is the mass of the melting ice.
An aluminum calorimeter with mass 85g and containing 310g of water are initially at thermal equilibrium at 20 ̊C (room temperature). An ice cube is taken from the freezer with T = –8.5 ̊C and placed in the calorimeter water. When all the ice is melted, the final temperature is 17 ̊C. The specific heat of Al is 900 J/kg ̊C, the specific heat of ice is 2100 J/kg ̊C, and of liquid water is 4186 J/kg ̊C. The latent heat of fusion of water is 3.3x105 J/kg. What was the original mass of the ice cube? You can calculate the original mass of the ice cube in several steps:
a) First calculate the total heat lost by the 85g calorimeter and the 310g of liquid water when they are cooled to 17 degrees C.
b) To calculate the ice mass, assume all the heat lost by the calorimeter and water from part (a) goes into heating the ice to 0 ̊C, melting the ice at 0 ̊C, and then raising the melted ice (now water) to +17 ̊C, in three steps. The only unknown is the mass of the melting ice.
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