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.

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.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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