Ethene (C2H4) can react with a halogen (for example, Cl2, Br2, or I2) by the following reaction: C2…

Ethene (C2H4) can react with a halogen (for example, Cl2, Br2, or I2) by the following reaction: C2H4 (g) + X2 (g) → C2H4X2 (g) Where X can be Cl, Br, or I. Using the thermodynamic data given below, determine which process you would expect to be the most spontaneous (i.e. which product would be most likely to form under standard conditions): C2H4Cl2, C2H4Br2, or C2H4I2. If the reactions were completed at higher temperatures, would the reactions be more or less spontaneous? Explain. Compound Standard Enthalpy of Formation (ΔHf°; kJ/mol) Standard Entropy (S°; J/(K mol)) C2H4Cl2 (g) -22.9 308.0 C2H4Br2 (g) -185.1 330.6 C2H4I2 (g) -11.3 347.8 C2H4 (g) 52.4 219.3 Cl2 (g) 0 223.1 Br2 (g) 30.9* 245.5 I2 (g) 62.4* 260.7 * Note: these are not 0 because the standard state for Br2 is a liquid, and I2 is a solid (not a gas)

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