Consider the following thermochemical equations: C (diamond) + O2 (g) --> CO2 (g) ΔH° = –395.4 kJ 2 CO2 (g) --> 2 CO (g) + O2 (g) ΔH° = 566.0 kJ C (graphite) + O2 (g) --> CO2 (g) ΔH° = –393.5 kJ 2 CO (g) --> C (graphite) + CO2 (g) ΔH° = –172.5 kJ Use the thermochemical equations as needed to find the heat of formation of diamond.
Consider the following thermochemical equations: C (diamond) + O2 (g) --> CO2 (g) ΔH° = –395.4 kJ 2 CO2 (g) --> 2 CO (g) + O2 (g) ΔH° = 566.0 kJ C (graphite) + O2 (g) --> CO2 (g) ΔH° = –393.5 kJ 2 CO (g) --> C (graphite) + CO2 (g) ΔH° = –172.5 kJ Use the thermochemical equations as needed to find the heat of formation of diamond.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section4.10: Standard Formation Enthalpies
Problem 4.18CE
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- Consider the following thermochemical equations:
C (diamond) + O2 (g) --> CO2 (g) ΔH° = –395.4 kJ
2 CO2 (g) --> 2 CO (g) + O2 (g) ΔH° = 566.0 kJ
C (graphite) + O2 (g) --> CO2 (g) ΔH° = –393.5 kJ
2 CO (g) --> C (graphite) + CO2 (g) ΔH° = –172.5 kJ
Use the thermochemical equations as needed to find the heat of formation of diamond.
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