Question

1. Determine the standard Gibb's free energy change for the conversion of diamond into graphite in...

1. Determine the standard Gibb's free energy change for the conversion of diamond into graphite in units of kJ/mol and is it spontaneous, nonspontaneous, or neither.

Cdiamond (s)  ? Cgraphite (s)

capital delta Gf° for diamond = 2.9 kJ/mol

capital delta Gf° for graphite = 0.0 kJ/mol (Please be careful wtih sig figs.)

2. For the following reaction, capital delta G degree = 68.1 kJ/mol:

2 C(s) + 2 H2(g) ? C2H4(g)

Determine capital delta G for the reaction in units of kJ/mol at 1800. K, a partial pressure of C2H2 of 0.010 atm, and a partial pressure of H2 of 0.98 atm. (Please be careful wtih sig figs.)

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Answer #1

1)


Given:
Gof(Cdiamond(s)) = 2.9 KJ/mol
Gof(Cgraphite(s)) = 0.0 KJ/mol

Balanced chemical equation is:
Cdiamond(s) ---> Cgraphite(s)

?Go rxn = 1*Gof(Cgraphite(s)) - 1*Gof( Cdiamond(s))
?Go rxn = 1*(0.0) - 1*(2.9)
?Go rxn = -2.9 KJ
Answer: -2.9 KJ
This is spontaneous because ?Go rxn is negative

Only 1 question at a time please

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Answer #2

1)


Given:
Gof(Cdiamond(s)) = 2.9 KJ/mol
Gof(Cgraphite(s)) = 0.0 KJ/mol

Balanced chemical equation is:
Cdiamond(s) ---> Cgraphite(s)

?Go rxn = 1*Gof(Cgraphite(s)) - 1*Gof( Cdiamond(s))
?Go rxn = 1*(0.0) - 1*(2.9)
?Go rxn = -2.9 KJ
Answer: -2.9 KJ
This is spontaneous because ?Go rxn is negative

Only 1 question at a time please

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