a) estimate the gas phase enthalpy using the bond dissociation enthalpies provid

Question

a) estimate the gas phase enthalpy using the bond dissociation enthalpies provided. b) is the reaction exothermic or endothermic? c) is the reaction likely to proceed spontaneously in the direction written?

For the reaction below: Cl CH CHCH CH3CHCH3 a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the owL Table Refere then click the Tables link on the drop-down that appears. Include algebraic sign and units 1208 b. Is the reaction exothermic or endothermic? endo v c. is the reaction likely to proceed spontaneously in the direction written? yes V more group attempts remaining Retry Entire Group

Explanation / Answer

For the given reaction,

a. dHrxn = dH(reactants) - dH(products)

               = 409 - 431

               = -22 kJ/mol

b. dHrxn is -ve so the reaction is exothermic in nature

c. The reaction would be spontaneous as written

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