Answer:
7598 J
Step-by-step explanation:
Solid ice has a specific heat capacity that is different from that of liquid water. The value of that is not given here, so we will assume that "liquid ice" has the same specific heat as liquid water.
The heat liberated by cooling 14 g of water from 30°C to -20°C is ...
(4.184 J)/(g·K)×(14 g)×(30-(-20))K = 2928.8 J
The mass 14 g of water in moles is ...
(14 g)/(18.01528 g/mol) ≈ 0.77712 mol
The heat of fusion (converting liquid water to "liquid ice") is then ...
(6.008 kJ)/mol × 0.77712 mol = 4668.9 J
So, the total amount of heat liberated by the change in temperature and form is ...
2928.8 J +4668.9 J ≈ 7598 J