4. The standard heat of forrmation of glycerine cannot be measured directly but can be determined indirectly from other heats of reaction by applying Hess's Law. Given the following data for the combustion of carbon, hydrogen, and glycerine, C,H;O3, in oxygen: C (s) + Ó2 (g) → CO2 (g) H2 (g) + ½ O2 (g) → H2O (I) C;H3O; + 3½ O2 (g) → 3 CO2 (g) +4 H2O (1) AH=-393.5 kJ AH=-285.8 kJ AH=-1.651 x 10³ kJ Calculate the standard heat of formation of glycerine.

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4.
The standard heat of forrmation of glycerine cannot be measured directly but can be determined
indirectly from other heats of reaction by applying Hess's Law. Given the following data for the combustion of
carbon, hydrogen, and glycerine, C;H&O3, in oxygen:
C (s) + O2 (g) → CO2 (g)
H2 (g) + /½ O2 (g) → H2O (1)
AH = -393.5 kJ
AH=-285.8 kJ
СЭH:Оз + 31/2 02 (g) —> 3 СО2 (g) + 4 H:0 (1)
ДН%--1.651 х 103 kJ
Calculate the standard heat of formation of glycerine.
Transcribed Image Text:4. The standard heat of forrmation of glycerine cannot be measured directly but can be determined indirectly from other heats of reaction by applying Hess's Law. Given the following data for the combustion of carbon, hydrogen, and glycerine, C;H&O3, in oxygen: C (s) + O2 (g) → CO2 (g) H2 (g) + /½ O2 (g) → H2O (1) AH = -393.5 kJ AH=-285.8 kJ СЭH:Оз + 31/2 02 (g) —> 3 СО2 (g) + 4 H:0 (1) ДН%--1.651 х 103 kJ Calculate the standard heat of formation of glycerine.
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