You add 50.0 grams of Ice at 0.0 °C to some warm water at 45.0 °C. All the Ice melts at constant 0.0 °C • All the water from the Ice warms from 0.0 °C to 10.0 °C (=Tfinal). • All the warm water cools to 10.0 °C (=Tfinal). How many grams of Warm Water did you start with? (Hint - three energies involved) • Specific Heat of Ice = 2.09 J/gºC • Specific Heat of Water = 4.184 J/gºC • Enthalpy of Fusion for Ice = 6.02 kJ/mol • Molar Mass of Water = 18.015 g/mol

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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You add 50.0 grams of Ice at 0.0 °C to some warm water at 45.0 °C.
All the Ice melts at constant 0.0 °C
• All the water from the Ice warms from 0.0 °C to 10.0 °C (=Tfinal).
• All the warm water cools to 10.0 °C (=Tfinal).
How many grams of Warm Water did you start with? (Hint - three energies involved)
• Specific Heat of Ice = 2.09 J/gºC
• Specific Heat of Water = 4.184 J/gºC
• Enthalpy of Fusion for Ice = 6.02 kJ/mol
• Molar Mass of Water = 18.015 g/mol
.
Transcribed Image Text:You add 50.0 grams of Ice at 0.0 °C to some warm water at 45.0 °C. All the Ice melts at constant 0.0 °C • All the water from the Ice warms from 0.0 °C to 10.0 °C (=Tfinal). • All the warm water cools to 10.0 °C (=Tfinal). How many grams of Warm Water did you start with? (Hint - three energies involved) • Specific Heat of Ice = 2.09 J/gºC • Specific Heat of Water = 4.184 J/gºC • Enthalpy of Fusion for Ice = 6.02 kJ/mol • Molar Mass of Water = 18.015 g/mol .
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