Answer:The enthalpy of fusion \((ΔH_f)\) of the sodium acetate is 12.344 kJ/mol.
Explanation:
Heat absorbed by the water: Q
Change in temperature of water,\(\Delta T=32.2^oC-25^oC=7.2^oC\)
Specific heat of water = 4.18 J/g°C
Mass of water = m= 500 g
\(Q=500 g\times 4.18 J/g ^oC\times 7.2^oC=15,048 J\)
\(\Delta H_f\) is the heat energy required to melt the one mole of substance.
When 200 g of sodium acetate crystallizes it gave 15,048 Joules of heat which was absorbed by the water in calorimeter.
\(NaAC(l)\rightarrow NaAC(s),\Delta H_f=?\)
Moles of NaAC=\(\frac{100 g}{82.03 g.mol}=1.2190 mol\)
\(\Delta H_f=\frac{15,048 J}{1.2190 mol}=12,344 J/mol=12.344 kJ/mol\)
The enthalpy of fusion \((ΔH_f)\) of the sodium acetate is 12.344 kJ/mol.
