A 34.0-g ice cube floats in 234 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 98.2°C is dropped into the cup, and the final equilibrium temperature is 12.0°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33 x 105 1/kg and 4,186 J/kg - °C, respectively. The specific heat of lead and copper are 128 J/kg - °C and 387 J/kg - °C, respectively.)

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A 34.0-g ice cube floats in 234 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 98.2°C is dropped into the cup, and the final equilibrium temperature is 12.0°C. What is the mass of the lead? (The heat of fusion and
specific heat of water are 3.33 x 105 1/kg and 4,186 J/kg · °C, respectively. The specific heat of lead and copper are 128 J/kg - °C and 387 J/kg - °C, respectively.)
Transcribed Image Text:A 34.0-g ice cube floats in 234 g of water in a 100-g copper cup; all are at a temperature of 0°C. A piece of lead at 98.2°C is dropped into the cup, and the final equilibrium temperature is 12.0°C. What is the mass of the lead? (The heat of fusion and specific heat of water are 3.33 x 105 1/kg and 4,186 J/kg · °C, respectively. The specific heat of lead and copper are 128 J/kg - °C and 387 J/kg - °C, respectively.)
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