Calculate the energy required to melt 12.4 g of ice at 0 oC.
The molar heat of fusion for ice is 6.02 kJ/mol.

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