At $700K$ acetaldehyde decomposes in the gas phase to methane and carbon monoxide. The reaction is:

$C{H}_3$CHO$(g)C{H}_4(g)+CO(g)$

A sample of $C{H}_3$CHO is heated to $700K$ and the pressure is measured as $220\frac{m}{b}ar$ before any reaction takes place. The kinetics of the reaction are then followed by measurements of total pressure and these data are obtained:

$\backslash$table$[[t(s),0,1000,3000,7000],[P_{\text{T}\text{o}\text{t}\text{a}\text{l}}($mbar$),220,240,270,310]]$

Part A

Find the rate law

Rate $=-\frac{P_{C{H}_3\text{C}\text{H}\text{O}}}{t}=()-1()-1$

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Part B

Find total pressure after $8\mathrm{.}00{10}^{4}s$

Express your answer to two significant figures and include the appropriate units.

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