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Heating Water and Ice: Energy Calculations for Temperature Changes and Phase Transitions

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This article explores the energy dynamics involved in heating water and ice through various temperature changes and phase transitions. We analyze three scenarios: heating 100 g of liquid water from 1.0˚C to 111˚C and calculating the energy added, heating solid water from -10.0˚C with 73.1 kJ of heat to find the final temperature, and examining the steam transformation process when 171 kJ of heat is added to water at 70.0˚C. The calculations utilize specific heat capacities and heat of fusion/vaporization to understand energy transfers.

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Heating Water and Ice: Energy Calculations for Temperature Changes and Phase Transitions

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Presentation Transcript

  1. Temperature (C) Time (s)

  2. Crossing the Line… 100.0 g of liquid water is heated from 1.0˚C to 111˚C. How much energy was added to the water to cause this temperature change? Cice = 2.1 J/g˚C Hfusion = 334 J/g Cwater =4.2 J/g˚C Hvap = 2260 J/g Csteam = 31.3J/g˚C

  3. Crossing the Line Again… 100.0 g of solid water is heated from -10.0˚C to some new temp. If 73.1 kJ of heat are added to the ice, what is the final temperature of the resulting material? Cice = 2.1 J/g˚C Hfusion = 334 J/g Cwater =4.2 J/g˚C Hvap = 2260 J/g Csteam = 31.3J/g˚C

  4. Crossing the Line One Last Time… 100.0 g of water at 70.0˚C is heated with a burner. If 171 kJ of heat are added to the water, what percentage of the water turns to steam? Cice = 2.1 J/g˚C Hfusion = 334 J/g Cwater =4.2 J/g˚C Hvap = 2260 J/g Csteam = 31.3J/g˚C

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