A 2.00 kg block of ice at -10.0 °C is placed in a large bucket of pure liquid water at 0.00 °C. When the system reaches equilibrium, there is still some liquid water left in the bucket at 0.00 °C. (Hint: At the instant the ice reaches 0°C it will be at thermal equilibrium and thus will immediately stop accepting heat) Cm,ice = 2090 J/kg·K, Cm, water = 4186 J/kg-K, Lf, water = 3.34 x 10$ J/kg
A 2.00 kg block of ice at -10.0 °C is placed in a large bucket of pure liquid water at 0.00 °C. When the system reaches equilibrium, there is still some liquid water left in the bucket at 0.00 °C. (Hint: At the instant the ice reaches 0°C it will be at thermal equilibrium and thus will immediately stop accepting heat) Cm,ice = 2090 J/kg·K, Cm, water = 4186 J/kg-K, Lf, water = 3.34 x 10$ J/kg
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Find the total mass of ice in the system when it reaches equilibrium.
Sketch two separate temperature vs. energy added diagrams (just a sketch, no numbers necessary!), one for the ice and one for the water. On each, draw and label two dots: one corresponding to the initial state and one corresponding to the final state.
For each substance (ice and water), determine from your diagrams if they undergo a temperature change, phase change, or both.
Transcribed Image Text:A 2.00 kg block of ice at -10.0 °C is placed in a large bucket of pure liquid water at 0.00 °C. When the system
reaches equilibrium, there is still some liquid water left in the bucket at 0.00 °C. (Hint: At the instant the ice
reaches 0°C it will be at thermal equilibrium and thus will immediately stop accepting heat)
Cm,ice = 2090 J/kg·K, Cm, water
= 4186 J/kg-K, Lf, water = 3.34 x 10$ J/kg
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