14. Diamond and graphite are two crystalline forms of carbon. At 1 atm and 25oC, diamond, changes to graphite so slowly that the enthalpy change of the process must be obtained indirectly. Using equations from the numbered list below, determine delta H forC(diamond) -> C(graphite)(1) C(diamond) + O2(g) -> CO2(g) ΔH = -395.4 kJ(2) 2CO2(g) -> 2CO(g) + O2(g) ΔH = 566.0 kJ(3) C(graphite) + O2(g) -> CO2(g) ΔH = -393.5 kJ(4) 2CO(g) -> C(graphite) + CO2(g) ΔH = -172.5 kJ

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Asked Nov 7, 2019

 

14. Diamond and graphite are two crystalline forms of carbon. At 1 atm and 25oC, diamond, changes to graphite so slowly that the enthalpy change of the process must be obtained indirectly. Using equations from the numbered list below, determine delta H for

C(diamond) -> C(graphite)

(1) C(diamond) + O2(g) -> CO2(g) ΔH = -395.4 kJ

(2) 2CO2(g) -> 2CO(g) + O2(g) ΔH = 566.0 kJ

(3) C(graphite) + O2(g) -> CO2(g) ΔH = -393.5 kJ

(4) 2CO(g) -> C(graphite) + CO2(g) ΔH = -172.5 kJ

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Step 1

According to the given question,

The enthalpy of formation of this reaction (ΔH) is calculated by Hess law.

Hess law states that “ regardless of multiple stages of the reaction, the total enth...

C(Dimond)C(Graphite)
2)
ΔΗ, -ΔΗ+ΔΗ, +ΔΗ, +.. .
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C(Dimond)C(Graphite) 2) ΔΗ, -ΔΗ+ΔΗ, +ΔΗ, +.. .

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