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Chemistry | 11th Edition | ISBN: 9780073402680 | Authors: Raymond Chang
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Calculate the standard enthalpy of formation of ClO from

Chapter 20, Problem 80P

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QUESTION:

Calculate the standard enthalpy of formation \(\left(\Delta H_{\mathrm{f}}^{\circ}\right)\) of ClO from the following bond enthalpies: \(\mathrm{Cl}_{2}\): 242.7 kJ/mol; \(\mathrm{O}_{2}\): 498.7 kJ/mol; ClO: 206 kJ/mol.

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QUESTION:

Calculate the standard enthalpy of formation \(\left(\Delta H_{\mathrm{f}}^{\circ}\right)\) of ClO from the following bond enthalpies: \(\mathrm{Cl}_{2}\): 242.7 kJ/mol; \(\mathrm{O}_{2}\): 498.7 kJ/mol; ClO: 206 kJ/mol.

ANSWER:

Step 1 of 3

We need to calculate the standard enthalpy of formation of


The energy that is released (or consumed) when one mole of a compound is created under standard conditions from its pure elements is the standard enthalpy of formation .

In the calculation of the standard enthalpy of formation , bond energies of bonds formed should be subtracted from the bonds that were broken. Bond energies should be multiplied with the corresponding stoichiometric coefficients.

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