Use the Gibbs-Free energy- Keq equation and determine the relationship of temperature with the ratio of partial pressure of PCl_{5} and Cl_{2}

Recall that Keq is similar to the ratio of PCl_{5}-Cl_{2}, recall that Keq can be written as:

$\overline{){\mathbf{Keq}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{{\mathbf{P}}_{\mathbf{products}}}{{\mathbf{P}}_{\mathbf{reactants}}}{\mathbf{=}}\frac{{\mathbf{P}}_{{\mathbf{PCl}}_{\mathbf{5}}}}{{\mathbf{P}}_{{\mathbf{Cl}}_{\mathbf{2}}}\mathbf{}\mathbf{\times}{\mathbf{P}}_{{\mathbf{Cl}}_{\mathbf{3}}}}}$

Thus, as __Keq increases, the ratio of PCl _{5}-Cl_{2 }also increases.__

Consider the following system at equilibrium at 25°C: PCl_{3}(g) + Cl_{2}(g) <=> PCl_{5}(g) for which ∆G° = -92.50 kJ. What will happen to the ratio of partial pressure of PCl_{5} to partial pressure of Cl_{2} as the temperature is raised?

a. increases

b. decreases

c. not affected

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