At 1 atm, how much energy is required to heat 37.0 g of H2O(s) at â€“10.0...

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Chemistry

At 1 atm, how much energy is required to heat 37.0 g of H2O(s)at â€“10.0 Â°C to H2O(g) at 169.0 Â°C? Helpful constants can be foundhere.
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/(gÂ·Â°C) * 37.60 J/(molÂ·Â°C) *
Specific heat of liquid H₂O (water) 4.184 J/(gÂ·Â°C) * 75.37 J/(molÂ·Â°C) *
Specific heat of gaseous H₂O (steam) 2.000 J/(gÂ·Â°C) * 36.03 J/(molÂ·Â°C) *

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3.7 Ratings (492 Votes)

This is calculated in 5 stages 1 To heat the ice from 10C to 0C dT 10C Q mcdT Q heat m mass of water 37 g c specific heat of ice 2087 JgC dT temperature See Answer

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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/(gÂ·Â°C) *	37.60 J/(molÂ·Â°C) *
Specific heat of liquid H₂O (water)	4.184 J/(gÂ·Â°C) *	75.37 J/(molÂ·Â°C) *
Specific heat of gaseous H₂O (steam)	2.000 J/(gÂ·Â°C) *	36.03 J/(molÂ·Â°C) *