Calculate the empirical formula for $E$.
In a suitable apparatus, $0.130\,\text{g}$ of $E$ was vaporised and took up $58.0\,\text{cm}^3$ at $127^{\circ}\text{C}$ and $1.00 \times 10^5\,\text{N m}^{-2}$. Use $pV = \frac{mRT}{M_r}$ to find $M_r$ of $E$, where $m$ represents the mass of $E$.
Therefore calculate the molecular formula of $E$.
Compound $F$ is an ester with molecular formula $\text{C}_4\text{H}_8\text{O}_2$. $F$ is one of four isomers, $S$, $T$, $U$, and $V$, and all of them are esters. The structural formula of $S$ is shown in the boxes below. Draw the structural formulae of the other three ester isomers of $F$.
When ester $F$ is hydrolysed, alcohol $G$ is formed. Which reagent can be used to hydrolyse an ester to an alcohol?
What other kind of organic compound is formed at the same time?
On mild oxidation, alcohol $G$ produces compound $H$ which gives a silver mirror with Tollens’ reagent. What functional group does the reaction with Tollens’ reagent show is present in compound $H$? Name this group.
What type of alcohol is $G$?
What could the structural formula of alcohol $G$ be?
Which of the four isomers, $S$, $T$, $U$, or $V$, could not be $F$?
Explain your answer.