The polymerisation of ethylene to linear polyethylene is represented by the reaction
`nCH_(2)=CH_(2)rarr(-CH_(2)-CH_(2)-)_(n)`
When `n` has a large integral value. Given theat the average enthalpies of bond dissociation for `C=C` and `C-C` at `298K`are `+590` and `+331kJ mol^(-1)` respectively, calculate the enthalpy of polymerisation per mole of ethylene at `298K`.

Explanation

To calculate the enthalpy of polymerization per mole of ethylene at 298 K, we can follow these steps:

### Step 1: Identify the bonds involved in the reaction
In the polymerization of ethylene (C₂H₄) to linear polyethylene, we start with n moles of ethylene, which means we have n C=C double bonds. When these double bonds are broken, they will form single C-C bonds in the polymer.

### Step 2: Determine the number of bonds broken and formed
- **Bonds broken**: There are n C=C double bonds in n moles of ethylene. Therefore, the total number of double bonds broken is n.
- **Bonds formed**: Each C=C double bond, when broken, will lead to the formation of 2 C-C single bonds. Thus, for n double bonds, we will form 2n C-C bonds.
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