Can someone check my answer? Thank you.
A calorimeter contains 500 g of water at 25°C. You place a hand warmer containing 200 g of liquid sodium acetate inside the calorimeter. When the sodium acetate finishes crystallizing, the temperature of the water inside the calorimeter is 39.4°C. The specific heat of water is 4.18 J/g-°C. What is the enthalpy of fusion (Hf) of the sodium acetate? (Show your work.) Where necessary, use q = mHf.

(4.18 J/g-C)(500 g)(39.4 - 25)C = 30,096 J
(30,096 J) divided by ((200 g C2H3NaO2) divided by (82.0338 g C2H3NaO2/mol))
=
30,096J divided by 2.438 mol

= 12,344 J/mol
or 12.344 kJ/mol

Question

Can someone check my answer? Thank you.
A calorimeter contains 500 g of water at 25°C. You place a hand warmer containing 200 g of liquid sodium acetate inside the calorimeter. When the sodium acetate finishes crystallizing, the temperature of the water inside the calorimeter is 39.4°C. The specific heat of water is 4.18 J/g-°C. What is the enthalpy of fusion (Hf) of the sodium acetate? (Show your work.) Where necessary, use q = mHf.

(4.18 J/g-C)(500 g)(39.4 - 25)C = 30,096 J
 (30,096 J) divided by ((200 g C2H3NaO2) divided by (82.0338 g C2H3NaO2/mol))
=
30,096J divided by  2.438 mol

= 12,344 J/mol 
or 12.344 kJ/mol