Calculate the standard change in Gibbs free energy for the following reaction at

Question

Explanation / Answer

Lancenigo di Villorba (TV), Italy The reaction involved is C(Graphite) + 2 Cl2(g) ---> CCl4(l) Its own STANDARD GIBB-FREE ENERGY's CHANGE follows DeltaG° = (G°f,CCl4) - (G°f,C + 2 * G°f,Cl2) = = (-203,344) - (0.0 + 2 * 0.0) = -203,344 J/mol Instead I use the FORMATION's GIBB-FREE ENERGY for Carbon Tetrachloride, I assumed NIHIL the other ones since they refer to MOST STABLE ALLOTROPIC STATES of Chemical Elements. The "Isothermal van't Hoff Equation" DeltaG = DeltaG° + R * T * SUM[nu,i * LN(a,i)] may be rearranged at the Equilibrium Conditions, e.g. where it is DeltaG = 0 and SUM[nu,i * LN(a,i)] = LN(Keq) so it is Keq = EXP(0 - DeltaG° / (R * T)) = = EXP(0 - (-203,344) / (8.3 * 298.16)) = 4.8E+35 I hope this could be clear.

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.