How many kJ are removed to convert 1.75 moles water from liquid at 0°C to solid at 0°C?

Question

I have a homework problem, and need help figuring out the answer. Show work if possible, please.

Latent Heat of Fusion of Water: ∆Hfus(H2O)= 80 calories/ gram= 334 Joules/gram.

Answer 1

(1.75 moles)(18 g/mole)(334 J/g)(1 kJ/1,000 J) =
10.521 kJ

Answer 2

Come on dog. If you had posted the latent heat of Ice for liquid to solid with your question, someone would have answered faster.

the latent heat of water from solid to liquid

Lsolid-liquid = 3.3 x 10/\5 J/kg 1.75 moles of water at 18 g / mol is about 31.5 g or .0315 kg

3.3 x 10/\5 J/kg * .0315 kg / 1000 = your answer