At 1 atm, how much energy is required to heat 81.0 g H2O(s)81.0 g H2O(s) at −22.0 ∘C−22.0 ∘C to H2O(g)H2O(g) at 123.0 ∘C?123.0 ∘C? Use the heat transfer constants found in this table. Heat-transfer constants for H2O at 1 atm Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H2O (steam) 2.000 J/(g·°C) * 36.03 J/(mol·°C) * *Specific heats change slightly with temperature. The values given in this table are a compromise among the accepted averages from several top-selling general chemistry textbooks. The slight differences in these values will not significantly affect your answers on homework problems.
At 1 atm, how much energy is required to heat 81.0 g H2O(s)81.0 g H2O(s) at −22.0 ∘C−22.0 ∘C to H2O(g)H2O(g) at 123.0 ∘C?123.0 ∘C? Use the heat transfer constants found in this table. Heat-transfer constants for H2O at 1 atm Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H2O (steam) 2.000 J/(g·°C) * 36.03 J/(mol·°C) * *Specific heats change slightly with temperature. The values given in this table are a compromise among the accepted averages from several top-selling general chemistry textbooks. The slight differences in these values will not significantly affect your answers on homework problems.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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At 1 atm, how much energy is required to heat 81.0 g H2O(s)81.0 g H2O(s) at −22.0 ∘C−22.0 ∘C to H2O(g)H2O(g) at 123.0 ∘C?123.0 ∘C? Use the heat transfer constants found in this table.
Heat-transfer constants for H2O at 1 atm
Quantity | per gram | per mole |
Enthalpy of fusion | 333.6 J/g | 6010. J/mol |
Enthalpy of vaporization | 2257 J/g | 40660 J/mol |
Specific heat of solid H2O (ice) | 2.087 J/(g·°C) * | 37.60 J/(mol·°C) * |
Specific heat of liquid H2O (water) | 4.184 J/(g·°C) * | 75.37 J/(mol·°C) * |
Specific heat of gaseous H2O (steam) | 2.000 J/(g·°C) * | 36.03 J/(mol·°C) * |
*Specific heats change slightly with temperature. The values given in this table are a compromise among the accepted averages from several top-selling general chemistry textbooks. The slight differences in these values will not significantly affect your answers on homework problems.
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