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The thermal decomposition of ethylene occurs in many industrial contexts: during ethylene transit in

pipelines, formation of polyethylene, drying of the gas, and separating it from impurities. The

decomposition reaction is as follows:

$C{H}_2=C{H}_2(g)C{H}_4(g)+C(graphite)$

If the decomposition of $1$ mole of ethylene with a gas density of $0\mathrm{.}215\frac{g}{m}L$ starts at $23C$ and the

temperature increases by $950K,$ what is the final pressure of the confined gas? $($Ignore the volume of

graphite and use the van der Waals equation.$)$