Answer:
2.943 °C temperature change from the combustion of the glucose has been taken place.
Explanation:
Heat released on combustion of Benzoic acid; :
Enthaply of combustion of benzoic acid = 3,228 kJ/mol
Mass of benzoic acid = 0.590 g
Moles of benzoic acid = [tex]\frac{0.590 g}{122.12 g/mol}=0.004831 mol[/tex]
Energy released by 0.004831 moles of benzoic acid on combustion:
[tex]Q=3,228 kJ/mol \times 0.004831 mol=15.5955 kJ=15,595.5 J[/tex]
Heat capacity of the calorimeter = C
Change in temperature of the calorimeter = ΔT = 2.125°C
[tex]Q=C\times \Delta T[/tex]
[tex]15,595.5 J=C\times 2.125^oC[/tex]
[tex]C=7,339.05 J/^oC[/tex]
Heat released on combustion of Glucose: :
Enthaply of combustion of glucose= 2,780 kJ/mol.
Mass of glucose=1.400 g
Moles of glucose =[tex]\frac{1.400 g}{180.16 g/mol}=0.007771 mol[/tex]
Energy released by the 0.007771 moles of calorimeter combustion:
[tex]Q'=2,780 kJ/mol \times 0.007771 mol=21.6030 kJ=21,603.01 J[/tex]
Heat capacity of the calorimeter = C (calculated above)
Change in temperature of the calorimeter on combustion of glucose = ΔT'
[tex]Q'=C\times \Delta T'[/tex]
[tex]21,603.01 J=7,339.05 J/^oC\times \Delta T'[/tex]
[tex]\Delta T'=2.943^oC[/tex]
2.943 °C temperature change from the combustion of the glucose has been taken place.
