C(diamond) + O;(g) → CO;(g) AH = -395.4 kJ 2 CO;(g) → 2 CO(g) + O; (g) AH = 566.0 kJ C(graphite) + O;(g)→ CO,(g) AH = -393.5 kJ 2 CO(g) → C(graphite) + CO,(g) AH® = -172.5 kJ
C(diamond) + O;(g) → CO;(g) AH = -395.4 kJ 2 CO;(g) → 2 CO(g) + O; (g) AH = 566.0 kJ C(graphite) + O;(g)→ CO,(g) AH = -393.5 kJ 2 CO(g) → C(graphite) + CO,(g) AH® = -172.5 kJ
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.151QP: Graphite is burned in oxygen to give carbon monoxide and carbon dioxide. If the product mixture is...
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Question
Use the following thermochemical equations as needed to find the heat of formation of diamond:
![C(diamond) + O,(g) → CO;(g)
AH = -395.4 kJ
2 CO:(g) →2 CO(g) + O, (g)
AH = 566.0 kJ
C(graphite) + O,(g)→ CO,(g)
AH = -393.5 kJ
2 CO(g) → C(graphite) + CO,(g) AH = -172.5 kJ](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F27eceac4-a847-4a89-975e-3c2b44a7bc6d%2Fb98016d9-04f5-42b3-a0cf-7e8cbd80aba9%2Ffihe5ig_processed.png&w=3840&q=75)
Transcribed Image Text:C(diamond) + O,(g) → CO;(g)
AH = -395.4 kJ
2 CO:(g) →2 CO(g) + O, (g)
AH = 566.0 kJ
C(graphite) + O,(g)→ CO,(g)
AH = -393.5 kJ
2 CO(g) → C(graphite) + CO,(g) AH = -172.5 kJ
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