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The heat energy associated with a change in temperature that does not involve a change in phase is given by
where q is heat in joules, m is mass in grams, s is specific heat in joules per gram-degree Celsius, J/(g⋅∘C), and ΔT is the temperature change in degrees Celsius. The heat energy associated with a change in phase at constant temperature is given by
where q is heat in joules, m is mass in grams, and ΔH is the enthalpy in joules per gram.
The constants for H2O are shown here:
Specific heat of ice: sice=2.09 J/(g⋅∘C)
Specific heat of liquid water: swater=4.18 J/(g⋅∘C)
Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g
Enthalpy of vaporization (H2O(l)→H2O(g)): ΔHvap=2250 J/g
How much heat energy, in kilojoules, is required to convert 52.0 g of ice at −18.0 ∘C to water at 25.0 ∘C ?
Express your answer to three significant figures and include the appropriate units
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