Consider the following equilibrium system: \[ \mathrm{COCl}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g}) \] A 10.00 L evacuated flask is filled with \( 0.4489 \mathrm{~mol} \mathrm{COCl}_{2}(\mathrm{~g}) \) at \( \mathbf{2 9 7 . 7} \mathrm{K} \). The temperature is then raised to 609.0 K , where the decomposition of \( \mathrm{COCl}_{2} \) gas takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask is 3.274 atm. What is the value of the equilbrium constant in terms of concentrations, \( \mathrm{K}_{\mathrm{c}} \), at \( \mathbf{6 0 9 . 0 \mathrm { K }} \) ? \[ \mathrm{K}_{\mathrm{C}}= \]
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