$\overline{){\mathbf{K}}_{\mathbf{c}}\mathbf{}\mathbf{=}\mathbf{}\frac{\mathbf{product}}{\mathbf{reactant}}}\phantom{\rule{0ex}{0ex}}{\mathbf{K}}_{\mathbf{c}}\mathbf{}\mathbf{=}\frac{\left[{C}_{2}{H}_{4}{X}_{2}\right]}{\left[{C}_{2}{H}_{4}\right]\left[{X}_{2}\right]}$

(a)

2 Cl_{2} (g)

2 C_{2}H_{4} (g)

8 C_{2}H_{4}Cl_{2} (g)

Ethene (C_{2}H_{4}) can be halogenated by the following reaction: C_{2}H_{4}(g) + X_{2}(g) ⇌ C_{2}H_{4}X_{2}(g)

where X_{2} can be Cl_{2} (green), Br_{2} (brown), or I_{2} (purple). Examine the three figures below representing equilibrium concentrations in this reaction at the same temperature for the three different halogens.

where X

Rank the equilibrium constants for these three reactions from largest to smallest.

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