Question

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.

C_{diamond (s)}  ? C_{graphite (s)}

_f^{° for diamond = 2.9 kJ/mol}

_f^{° for graphite = 0.0 kJ/mol (Please be careful wtih sig figs.)}

2. For the following reaction, = 68.1 kJ/mol:

2 C_(s) + 2 H_2(g) ? C₂H_4(g)

Determine 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.)

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

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