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Question
The polymerization of propene is linear. Polypropene is represented by the reaction
Where n has large integral value, the average enthalpies of bond dissociation for (C = C) and (C - C) at 298 K are +590 and +331 KJ mol−1 respectively. The enthalpy of polymerization is −360 KJ mol−1. Find the value of n.___
Where n has large integral value, the average enthalpies of bond dissociation for (C = C) and (C - C) at 298 K are +590 and +331 KJ mol−1 respectively. The enthalpy of polymerization is −360 KJ mol−1. Find the value of n.
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Solution
Energy released = Energy input due to the double bond breaking -Energy due to formation of two single bonds:
2×331=662 KJ mol−1 of propene
ΔH polymerization/mol =590−662=−72 KJ mol−1
ΔH polymerization =−72×n=−360
n=5
2×331=662 KJ mol−1 of propene
ΔH polymerization/mol =590−662=−72 KJ mol−1
ΔH polymerization =−72×n=−360
n=5
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