Answer:The enthalpy of fusion [tex](ΔH_f)[/tex] of the sodium acetate is 12.344 kJ/mol.
Explanation:
Heat absorbed by the water: Q
Change in temperature of water,[tex]\Delta T=32.2^oC-25^oC=7.2^oC[/tex]
Specific heat of water = 4.18 J/g°C
Mass of water = m= 500 g
[tex]Q=500 g\times 4.18 J/g ^oC\times 7.2^oC=15,048 J[/tex]
[tex]\Delta H_f[/tex] 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.
[tex]NaAC(l)\rightarrow NaAC(s),\Delta H_f=?[/tex]
Moles of NaAC=[tex]\frac{100 g}{82.03 g.mol}=1.2190 mol[/tex]
[tex]\Delta H_f=\frac{15,048 J}{1.2190 mol}=12,344 J/mol=12.344 kJ/mol[/tex]
The enthalpy of fusion [tex](ΔH_f)[/tex] of the sodium acetate is 12.344 kJ/mol.
