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At 1 atm, how much energy is required to heat 73.0 g of H2O(s) at –22.0...

At 1 atm, how much energy is required to heat 73.0 g of H2O(s) at –22.0 °C to H2O(g) at 115.0 °C?

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At 1 atm, how much energy is required to heat 73.0 g of H2O(s) at –22.0...
At 1 atm, how much energy is required to heat 73.0 g of H2O(s) at –22.0 °C to H2O(g) at 121.0 °C?
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At 1 atm, how much energy is required to heat 55.0 g of H2O(s) at –22.0 °C to H2O(g) at 151.0 °C? 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) *
At 1 atm, how much energy is required to heat 55.0g of H2O(s) at -22.0 ^degree...
At 1 atm, how much energy is required to heat 55.0g of H2O(s) at -22.0 ^degree C to H2O(g) at 169.0^degree C?
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