Answer:
The enthlapy of solution is -55.23 kJ/mol.
Explanation:
Mass of water = m
Density of water = 1 g/mL
Volume of water = 50.0 mL
m = Density of water × Volume of water = 1 g/mL × 50.0 mL=50.0 g
Change in temperature of the water ,ΔT= 27.0°C - 22.3°C = 4.7°C
Heat capacity of water,c =4.186 J/g°C
Heat gained by the water when an unknown compound is dissolved be Q
Q= mcΔT
[tex]Q=50.0 g\times 4.186 J/g^oC\times 4.7^oC=983.71 J[/tex]
heat released when 0.9775 grams of an unknown compound is dissolved in water will be same as that heat gained by water.
Q'=-Q
Q'= -983.71 J =-0.98371 kJ
Moles of unknown compound = [tex]\frac{0.9975 g}{56 g/mol}=0.01781 mol[/tex]
The enthlapy of solution :
[tex]\frac{Q'}{moles}[/tex]
[tex]=\frac{-0.98371 kJ}{0.01781 mol}=-55.23 kJ/mol[/tex]
The enthlapy of solution is -55.23 kJ/mol.
