The molar heat of fusion for water is 6.008kJ/mol. How much energy would be required to melt 94.0g of ice?

31.36 kj

Explanation:

Given data:

Molar heat of fusion for water = 6.008 kj/mol

Energy required to melt 94 g ice = ?

Solution:

Number of moles of ice = mass/ molar mass

Number of moles = 94 g/ 18 g/mol

Number of moles = 5.22 mol

Energy required for one mole  = 6.008 kj

Energy required for 5.22 mole,

5.22 mol × 6.008 kj/ 1mol

31.36 kj

it takes on an electronical energy

b. is the answer hoped i