A 5.00 g sample of H2O is removed from a freezer and heated from an initial...

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Chemistry

A 5.00 g sample of H2O is removed from a freezer and heated froman initial temperature of -5.00 oC through to a final temperatureof 102.0 oC.
(a) Given the following data, calculate the amount of energythat has to be absorbed by the H2O during the whole process.
Freezing point of H2O = 0.00oC;
Boiling point of H2O = 100.oC
Î”Hfusion of H2O = 6.01 kJ mol-1
Î”Hevaporation of H2O = 40.7 kJ mol-1
Specific heat capacity of ice = 2.05 J g-1 K-1;
Specific heat capacity of water = 4.18 J g-1 K-1
Specific heat capacity of steam = 2.08 J g-1 K-1
(b) Calculate the percentage of the total energy required forthe overall process in (a) that is used just in heating the liquidwater.
(c) Calculate the mass of ice at 0.00oC, that can be melted in30 minutes by a heater that produces 8000 kJ of energy per hour butin such a way that only 70% of the heat produced is absorbed by theice.

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4.1 Ratings (677 Votes)

We know that 1 kJ1000 J Molar mass of H2O2xmolar mass of HMolar mass of O 2x1 gmol16 gmol 2 gmol16 gmol 18 gmol Number of moles in 500 g H2OGiven massmolar mass 500 g18 gmol0278 mol Amount of heat energy absorbed by water in the whole process Heat absorbed by ice to increase the temperature to 0C Heat absorbed to melt ice at 0C Heat absorbed to increase the temperature of liquid water to 100C Heat absorbed to vapourize See Answer

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