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

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

Given the information in figure 14.21, determine:
ΔSo, ΔHo, ΔGo for the following reaction at 25oC:

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, ΔSo = So of COCl2 - (So of CO + So of Cl2)
So, ΔSo = 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,ΔHo = ΔHof of COCl2 - (ΔHof of CO + ΔHof of Cl2)
So, ΔHo = -53.3 -(-26.4 + 0) = -53.3 + 26.4 = -26.9 Kcal = -26900 cal.

Change in Gibbs free energy = ΔGo = ΔHo - TΔSo where T is temperature in degree Kelvin.
So, ΔGo = -26900 - 298(-31.5) = -17513 = -17.5 Kcal.

The values of ΔSo, ΔHo, ΔGo are all negative. This indicates that this reaction will be spontaneous at low temperature.


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