At 1 atm, how much energy is required to heat 81.0 g of H2O(s) at –20.0...
At 1 atm, how much energy is required to heat 81.0 g of H2O(s) at –20.0 °C to H2O(g) at 149.0 °C? Helpful constants can be found here.
These are the helpful constants:
| 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) * |
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At 1 atm, how much energy is required to heat 81.0 g of H2O(s)
at –20.0...
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