Balance the half-equation for this reaction so that you can determine how many moles of electrons are needed to reduce 1 mole of nitrobenzene. $\mathrm{C_6H_5NO_2 + \dots e^- + \dots H^+ \rightarrow C_6H_5NH_2 + \dots H_2O}$
The usual reducing agent is granulated tin together with concentrated hydrochloric acid. In the first stage, the reduction of nitrobenzene to phenylammonium chloride is shown by the equation below. Use oxidation numbers or transferred electrons to balance this equation. $\mathrm{\dots C_6H_5NO_2 + \dots HCl + \dots Sn \rightarrow \dots C_6H_5NH_3Cl + \dots SnCl_4 + \dots H_2O}$
When $5.0\,\text{g}$ of nitrobenzene was reduced in this reaction, $4.2\,\text{g}$ of phenylammonium chloride, $\mathrm{C_6H_5NH_3Cl}$, was formed. Calculate the percentage yield.
After the reaction in (b), excess $\mathrm{NaOH(aq)}$ was added to free phenylamine from phenylammonium chloride. Calculate the mass of phenylamine, $\mathrm{C_6H_5NH_2}$, formed when $4.20\,\text{g}$ of phenylammonium chloride reacts with excess $\mathrm{NaOH(aq)}$.
In (i), the final volume of the alkaline phenylamine solution was $25.0\,\text{cm}^3$. Phenylamine was extracted by adding $50\,\text{cm}^3$ of dichloromethane. After extraction, the dichloromethane layer contained $2.68\,\text{g}$ of phenylamine. Use these data to calculate the partition coefficient, $K_{\text{partition}}$, of phenylamine between dichloromethane and water.
Compare the basicity of phenylamine with that of ethylamine. Explain your answer.
Phenol can be prepared from phenylamine in two steps. State the reagents and conditions for steps 1 and 2.
Draw the structure of intermediate compound $E$.