Change In Entropy, Enthalpy And Gibbs Free Energy In The Synthesis Reaction Of Carbon-Monoxide And Chlorine

Change In Entropy, Enthalpy And Gibbs Free Energy In The Synthesis Reaction Of Carbon-Monoxide And Chlorine
TECTechnics Classroom TECTechnics Overview

Entropy, Enthalpy, Free Enegy Changes In COrbon Monoxide -Chlorine Reaction

Given the information in figure 14.21, determine:
ΔS^o, ΔH^o, ΔG^o for the following reaction at 25^oC:

CO(g) + Cl₂(g) -------> COCl₂(g)

The strings:

S₇P₅A₅₂ (Change - Chemical Change)

The math:
Pj Problem of Interest is of type change (entropy change). Entropy, enthalpy and Gibbs free energy are state variables and the problem of interest is the change in these states as a result of the systhesis reaction of CO and Cl₂.

Entropy, Enthalpy, Free Enegy Changes In Carbon Monoxide-Chlorine Reaction

Change in entropy = Entropy of products - entropy of reactancts
So, ΔS^o = S^o of COCl₂ - (S^o of CO + S^o of Cl₂)
So, ΔS^o = 69.1 -(47.3 + 53.3) = -31.5 cal/mole-^oK

Change in enthalpy = Enthalpy of formation of products - enthalpy of formation of reactants
So,ΔH^o = ΔH^o_f of COCl₂ - (ΔH^o_f of CO + ΔH^o_f of Cl₂)
So, ΔH^o = -53.3 -(-26.4 + 0) = -53.3 + 26.4 = -26.9 Kcal = -26900 cal.

Change in Gibbs free energy = ΔG^o = ΔH^o - TΔS^o where T is temperature in degree Kelvin.
So, ΔG^o = -26900 - 298(-31.5) = -17513 = -17.5 Kcal.

The values of ΔS^o, ΔH^o, ΔG^o are all negative. This indicates that this reaction will be spontaneous at low temperature.

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