Estimate ΔHrxn for the following chemical reaction
using the bond enthalpies in the table found here. Report your
answer to zero decimal places in standard notation (i.e. 123. kJ
*For numbers ending in zero, be sure to include the
decimal!*).
C2H2(g) + Cl2(g) →
C2H2Cl2(g)
H rxn = H products - H reactants
H0 for ethene = +52.4 KJ/mole
H0 for Cl2 = 0 KJ/mole
H0 for ethylene chloride = -125.4 KJ/mole
Therefore, H rxn = H products - H reactants
H rxn = -125.4 - (52.4+0) = 73..0 KJ/mole
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