Question

part a spontaneity

What can be said about the spontaneity ofthis reaction?

$\rm C_{diamond} \rightarrow C_{graphite}$

The reaction (as written) is spontaneous. The reverse reaction is spontaneous. the system is in equilibrium at 298 K.

Part b

What is the standard Gibbs free energy forthis reaction?

${\Delta G_{\rm rxn}}^\circ$ =		$\rm kJ/mol$

Part c

What is the Gibbs free energy for thisreaction at 3200 $\rm K$ ? Assume that and do not change withtemperature.

${\Delta G_{\rm rxn}}$ =		$\rm kJ/mol$

Part d

At what temperature $T_eq$ do the forward and reverserusting reactions occur in equilibrium?

Express your answer in kelvins.

Answer 1

We Know that :

     The given Reaction is :

                

            The Reaction is Spontaneous as written in thegiven direction.

     

         ΔG_reaction   = ΔG⁰_products - ΔG⁰_reactants

                            = 0 - 2.900 KJ

                             =   - 2.900 KJ

          ΔG_reaction   = Δ H - TΔ S

                              = - 1.8 KJ - 3200 K x 3.223 J / K

                              = - 12.1136 KJ

          We Knowthat at equilibrium :

             Δ G = 0

           T_equilibrium   =   Δ H / Δ S