5. Consider the process of converting graphite to diamond: a. Calculate the change in enthalpy associated with converting graphite to diamond under standard conditions (T = 298 K, P = 1 bar) b. Calculate the change in entropy of this process. c. Calculate the change in Gibbs free energy of this process.
5. Consider the process of converting graphite to diamond: a. Calculate the change in enthalpy associated with converting graphite to diamond under standard conditions (T = 298 K, P = 1 bar) b. Calculate the change in entropy of this process. c. Calculate the change in Gibbs free energy of this process.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
5. Consider the process of converting graphite to diamond:
a. Calculate the change in enthalpy associated with converting graphite to diamond under
standard conditions (T = 298 K, P = 1 bar)
b. Calculate the change in entropy of this process.
c. Calculate the change in Gibbs free energy of this process.
d. Is this process spontaneous?
e. At what temperature will this process change spontaneity (i.e. becomes non-spontaneous
or becomes spontaneous)?
Transcribed Image Text:AH' (kJ/mol)
Sm (J/Kmol)
Diamond
2.391
2.337
Cgraphite → Cdiamond
Graphite
0
5.740
Expert Solution
Step 1
Given :
∆fH°( diamond) = 2.391 KJ/mol
∆fH°(graphite) = 0 KJ/mol
Sm (diamond) = 2.337 J/Kmol
Sm(graphite) = 5.740 J/Kmol
T = 298 K
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