At 1 atm, how much energy is required to heat 55.0 g H,O(s) at -16.0 °C to H,O(g) at 159.0 °C? Use the heat transfer constants found in this table. q = kJ

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Question 8 of 15
At 1 atm, how much energy is required to heat 55.0 g H,O(s) at –16.0 °C to H, O(g) at 159.0 °C? Use the heat transfer
constants found in this table.
kJ
q =
Transcribed Image Text:O Resources LX Give Up? O Hint Check Answer Question 8 of 15 At 1 atm, how much energy is required to heat 55.0 g H,O(s) at –16.0 °C to H, O(g) at 159.0 °C? Use the heat transfer constants found in this table. kJ q =
dix
Heat Transfer
Heat-transfer constants for H2O at 1 atm
Quantity
Enthalpy of fusion
Enthalpy of vaporization
Specific heat of solid H, 0 (ice)
per gram
per mole
333.6 J/g
6010. J/mol
2257 J/g
40660 J/mol
2.087 J/(g °C) * 37.60 J/(mol-°C) *
Specific heat of liquid H 2 0 (water)
4.184 J/(g-°C)
75.37 J/(mol-°C) *
Specific heat of gaseous H 2 O (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:
general chemistry textbooks. The slight differences in these values will not significantly affect your answers on homework problems.
ats
search
近
Transcribed Image Text:dix Heat Transfer Heat-transfer constants for H2O at 1 atm Quantity Enthalpy of fusion Enthalpy of vaporization Specific heat of solid H, 0 (ice) per gram per mole 333.6 J/g 6010. J/mol 2257 J/g 40660 J/mol 2.087 J/(g °C) * 37.60 J/(mol-°C) * Specific heat of liquid H 2 0 (water) 4.184 J/(g-°C) 75.37 J/(mol-°C) * Specific heat of gaseous H 2 O (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: general chemistry textbooks. The slight differences in these values will not significantly affect your answers on homework problems. ats search 近
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