Answer:
Energy required is 4.147 kj.
Explanation:
Given data:
Mass of ice = 12.4 g
Temperature = 0°C
Molar heat fusion for ice = 6.02 kj/mol
Energy required to melt = ?
Solution:
Formula:
q = n ×ΔH
q = heat
n = number of moles
ΔH = enthalpy
First of all we will calculate the number of moles.
Number of moles = mass/ molar mass
Number of moles = 12.4 g/ 18 g/mol
Number of moles = 0.69 mol
Now we will put the values in formula.
q = n × ΔH
q = 0.69 mol × 6.02 kj/mol
q = 4.147 kj
