A student ran the following reaction in the laboratory at 581 K: COCl2(g) CO(g) + Cl2(g) When he introduced COCl2(g) at a pressure of 0.872 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of Cl2(g) to be 0.390 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp =

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Electron equations of the given changes are as follow,a)                              cu      →      cu⁺²  + 2e⁻b)                              mg⁺²  +  2 e⁻      →      mgc)                              cl⁻    →      cl  +  1e⁻d)                              s  +  2 e⁻    →      s²⁻e)                                o²⁻      →      o  +  2 e⁻f)                              p  +  3 e⁻    →      p³⁻g)                              fe²⁺    →      fe³⁺  + 1 e⁻h)                              s²⁻    →      s⁴⁺  +  6 e⁻

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