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Sagot :
The energy required to melt 20 kg of ice at 0°C is 6.68 kJ.
The enthalpy change for melting of an ice is called the enthalpy of fusion. Its value is 6.02 kJ/mol. This means for every mole of ice we must apply 6.02 kJ of heat for melting. The calculation of heat is done by following equation.
q = n×ΔH
- q is heat
- n is number of moles
- ΔH is change in enthapy
in this problem we need to calculate heat needed to melt 20grams of ice at 0°C .
Calculation of moles of water,
Number of moles of water (n) = given mass/ molar mass = 20g/18.02g/mol
Number of moles of water (n) = 1.109 mole
heat or energy required = q = n×ΔH = 1.109 mole× 6.02 kJ/mol = 6.68 kJ
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