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12 Dec 2019

PLEASE HELP CHEMISTRY HOMEWORK ON THERMODYNAMICS DUE MONDAY EVENING, KINDLY SHOW ALL WORKS AND CALCULATIONS!!!

(11). C (diamond) Ã C (graphite)

For the reaction represented above, the standard Gibbs free energy change, ΔG°, has a value of -2.90 kJ/mol. Explain the observation that the reaction does NOToccur
(e.g., diamond is stable) at 298 K and 1.00 atm?

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Jean Keeling
Jean KeelingLv2
13 Dec 2019

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Related questions

Diamond
a. At 298 K, what is the Gibbs free energy change G for the following reaction? Cgraphite -> ïƒ Cdiamond

b. Is the diamond thermodynamically stable relative to graphite at 298 K?

c. What is the change of Gibbs free energy of diamond when it is compressed isothermally from 1 atm to 1000 atm at 298 K?

d. Assuming that graphite and diamond are incompressible, calculate the pressure at which the two exist in equilibrium at 298 K.


e. What is the Gibbs free energy of diamond relative to graphite at 900 K? Assume the heat capacities of the two materials are equal.


f. Diamond is synthesized from graphite at high pressures and high temperatures. The need for high pressure should be obvious from your calculations, but why is the process carried out at high temperature?


DATA
Density of graphite is 2.25 g/cm3 Density of diamond is 3.51 g/cm3

Delta Hf(298K) So(298K)
Diamond 1.897 kJ/mol 2.38 J/(K mol)
Graphite 0 5.73 J/(K mol)

Hf(298 K)S0

298 K

Diamond 1.897 kJ/mol 2.38 J/(K mol)

Graphite 0 5.73 J/(K mol)

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